# Synthesis Characterization and Biological Activity Study of New Schiff and Mannich Bases and Some Metal Complexes Derived from Isatin and Dithiooxamide

Authors: Ahlam J. Abdulghani; Nada M. Abbas
Journal: Bioinorganic Chemistry and Applications
 (2011)

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## Abstract

Two new Schiff and Mannich bases, namely, 1-Morpholinomethyl-3(1′ -N-dithiooxamide)iminoisatin (LIH) and 1-diphenylaminomethyl-3-1′-N-dithiooxamide)iminoisatin (LIIH), were prepared from condensation reaction of new Schiff base 3-(1′-N-dithiooxamide)iminoisatin (SBH)  with morpholine or diphenylamine respectively in presence of formaldehyde . The structures were characterized by IR, 1HNMR, mass spectrometry, and CHN analyses. Metal complexes of the two ligands were synthesized,  and their structures were characterized by elemental analyses, atomic absorption, IR and UV-visible spectra, molar conductivity,  and magnetic moment determination. All complexes showed octahedral geometries except palladium complexes which were square planar. The biological activity of the  prepared compounds and some selected metal complexes was tested  against three types of bacteria and against cell line of human epidermoid larynx carcinoma (Hep-2).


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## Body

## 1. Introduction

Various Mannich Schiff bases of isatin have been found to be of biological importance [1] and have shown anticonvulsant [2], antibacterial [3, 4], antimicrobial [5–7] and anti-HIV activities [8, 9]. Dithiooxamide (dto)  is an effective flexidentate complexing agent with varied coordination chemistry. Due to the intense chromophoric character, dto can be used in an imaging processes [10], coordination polymers [11], histological agents, and as a source for duplicating processes [12]. The transition metal complexes of dto and its derivatives are characterized by semiconductor, magnetic, and spectroscopic properties [12–15]. The aim of this work is to  synthesize and study the coordination behavior of the two new Schiff and Mannich base ligands LIH and LIIH shown in Scheme 1, from condensation reaction of a new Schiff base 3-(1′-N-dithiooxamide) iminoisatin (SBH) with morpholine or diphenylamine, respectively, in presence of formaldehyde in a mole ratio of (1 : 1 : 1), respectively, or from reaction of Mannich bases N-morpholinomethyl isatin (MI) and N-diphenylaminomethyl isatin (MII) [16] with dithiooxamide. The  biological activity of the two ligands and some of their metal complexes was investigated against selected types of bacteria and against cancer cell line of human epidermoid larynx carcinoma (Hep-2).Scheme 1
The structures of the prepared ligands.


## 2. Experimental/Materials and Methods

Melting points (uncorrected) were determined by using Gallenkamp MFB600–010f m.p apparatus. The purity of the synthesized compounds was checked by T.L.C. techniques using a mixture of chloroform and acetone (2 : 2 V/V) and various ratios of methyl acetate: acetone solvent mixture as eluents and iodine chamber for spot location. The HPLC of the Schiff base (SBH) and the derived two ligands were obtained by using HPLC (LKB), mobile phase CH3CN : H2O (80 : 20). Infrared spectra were recorded on a Perkin-Elmer 1310 IR spectrophotometer and Shimadzu corporation 200–91527 IR spectrophotometer using KBr and CsI disks. 1H n.m.r spectra of the organic compounds were recorded on a 300 MHz n.m.r spectrophotometer (Joel) using TMS as internal reference. Mass spectra were recorded on a Joel 700 mass spectrometer. Elemental CHN analyses were obtained by using EA elemental analyzer (Fison Ision Instrument). Electronic spectra of the ligands and their metal complexes in the region 200–1100 nm were recorded on a Shimadzu UV-visible-160 spectrophotometer. The metal contents were determined by atomic absorption technique using a Varian-AA-775 atomic absorption instrument. Electrical conductivity of metal complexes was measured at room temperature in DMF (10−3 M) using Elkta Lictfahigkeit conductivity meter (SIMENS). Magnetic moments (μeff BM) for the solid metal complexes at room temperature were determined according to Faraday’s method by using Johnson Mattey magnetic balance system division. Chloride content of metal complexes was determined by potentiometric titration using 1686-titroprocessor-665 Dosinametrom (Swiss). All organic and inorganic materials were of high purity and used as received except ethanol, methanol, and DMF which were dried and distilled prior to use [17]. Palladium(II) chloride was converted to dichlorobis(benzonitrile)palladium(II) [18], and H2PtCl6·6H2O was converted to potassium hexachloroplatinate(IV) hexahydrate [19] prior to use. Mannich bases N-morpholinomethylisatin (MI) and N-diphenylaminomethyl isatin (MII) were prepared according to methods mentioned in the literature [16]. Complex formation was  studied in solutions to obtain the molar ratio of the ligand to metal ion (L : M) using ethanol, or DMSO as solvents. A series of solutions containing constant concentration of the metal ion (1 × 10−4M) were treated with various amounts of the same concentration of the ligand. The results of (L : M) ratio were obtained by plotting absorbance of solution mixtures at detected λmax against [L]/[M].


## 3. Preparation of Ligands

### 3.1. 3-(1′-N-dithiooxamide)iminoisatin (SBH)

A solution mixture of isatin (0.01 mole, 1.47 g) and dto (0.01 mole, 1.021 g) in dry ethanol (50 mL) containing 2-3 drops glacial acetic acid was heated under reflux for 8 h with continuous stirring. The mixture was then left at room temperature for 24 hs. A yellow precipitate was formed. The product was filtered, washed with warm ethanol, and crystallized from ethanol:dichloromethane solvent mixture (1 : 1). m.p. 190°C yield 60%; IR (KBr)ν(cm−1): 3296, 3203 (NH2); 3147 (NH-isatin); 1733 (C=O), 1614 (−C=N); 1540 (C–S + δNH, I); 1430 (C–N + C–S, II); 1197 (C–S, III); 835 (C=S, IV). 1H n.m.r. δ(ppm) (CD2Cl2)  12.012 (1H, s, NH); 7.653–6.94 (4H, m, aromatic); 2.022 (2H, d, NH2). MS, (m/z) (I%) (EI) calculated for C10H7N3OS2 m.wt 249 g/mole: 250 (10) [M+1]; 221 (3.2) [M–CO]; 207 (4) [M–NCO]; 162 (2); 119 (24); 90 (7.5).


### 3.2. 1-Morpholinomethyl-3-(1′-N-dithiooxamide)iminoisatin (LIH) and 1-diphenylaminomethyl-3-1′-N-dithiooxamide)Iminoisatin (LIIH)

(a) To a stirred solution of 3-(1′-N-dithiooxamide)iminoisatin (SBH) (0.01 mole, 2.49 g) and formaldehyde 37% (0.015 mole) in warm dry ethanol (20 mL) was added, drop by drop, (0.01 mole) of morpholine (LIH) or diphenylamine (LIIH). The mixture was heated under reflux for 3 h with continuous stirring, and then left to cool at room temperature. A solid precipitate was formed. The products were filtered, washed with warm ethanol, and then crystallized from ethanol : chloroform (1 : 1 v/v) mixture; yield 35 and 28.2%, respectively.(b) To a solution of dto (5 mmole, 0.6 g) in warm ethanol (10 mL) containing 2-3 drops glacial acetic acid was added (5 mmole) of Mannich base N-Morpholinomethylisatin (MI) or N-Diphenylaminomethyl isatin (MII) [16] in ethanol (10 mL) with continuous stirring, and the mixture was heated under reflux for 10 h. After leaving the mixture at room temperature for 24 h a precipitate was formed. The products were filtered, washed with warm ethanol, and crystallized; yield 20.3 and 21%, respectively (m.p. 215 and 283°C, resp.).1-Morpholinomethyle-3-(1′-N-dithiooxamide)iminoisa- tin (LIH):
yellowish orange crystals, m.p. 162°C; IR (KBr).ν(cm−1): 3203, 3138 (NH2); 3030–3000 (arom CH); 2815–2364 (CH2); 1730 (C=O); 1614 (−C=N); 1589 (C=C arom.); 1540 (νC=N, δNH, I); 1429 (C–N + C–S, II); 1195 (C–S, III); 835 (C=S, IV); 1149, 1328 (morpholine). 1H n.m.r δ(ppm) (DMSO): 7.59-6.898 (4H, m, aromatic +NH); 4.09 (2H, d, N–CH2N); 3.65 (4H, d, 2”, 6” CH2 morph.); 2.33 (4H, d, 3”, 5” CH2 morph.); 1.567 (1H, br, SH). MS (FAB) m/z (I%) calculated for C15H16N4O2S2, m.wt 348.45 g/mole,: 349.1 (93) [M]; 320 (38) [M–CO]; 235 (100); 234 (80); 220 (15), 207 (40). 131 (43); 104 (78%); (EI) m/z (I%): 348.5 (84) [M]; 320 (25) [M–CO]; 234 (38); 207 (17); 130 (19); 117 (24);  104 (57); 90 (30); 78 (22%). CHN% Calculated for C15H16N4O2S2 C, 51.67; H, 4.59, N, 16.07% found C, 50.69; H, 4.20; N, 15.75%; νmax (cm−1) (DMF) (εmax mol−1 cm−1) 34013 (20030) π→π*; 2415 (2980), n→π* (DMSO) 38461 (19519) π→π*.Diphenylaminomethyl-3-(1′-N-dithiooxamide)Iminoisa tin (LIIH):
yellow red crystals, m.p. 182, IR (KBr)ν(cm−1): 3193, 3034 (NH2); 1730 (C=O); 1614 (C=N); 1540, 1434, 1195, 833 (C–N + δNH, C–N + C–S, C–S, C=S I–IV, resp.). 1H n.m.r (δ, ppm) (CD2Cl2): 7.59–6.89 (14H, m, aromatic); 4.83 (2H, d, CH2); 2.17 (2H, b, NH2). MS m/z (I%) (EI): calculated for C23H18N4OS2, m.wt 430.55 g/mol: 430.9 (5.5) [M]; 402 (2.5) [M–CO]; 235 (21); 129.2 (1.8);  104 (4.8); 89 (10.3); 78.1 (3.5%). CHN (%) calculated for C23H18N4OS2: C, 64.18, H, 4.21; N, 13.02% found: C, 64.02; H, 4.22; N, 13.52%. νmax (cm−1) (DMF) (εmax, L mol−1 cm−1) 32258 (22970) π→π*; 24509 (3530) n→π*; (DMSO): 38461 (19540): 28571 (14120) π→π*.


## 3.1. 3-(1′-N-dithiooxamide)iminoisatin (SBH)

A solution mixture of isatin (0.01 mole, 1.47 g) and dto (0.01 mole, 1.021 g) in dry ethanol (50 mL) containing 2-3 drops glacial acetic acid was heated under reflux for 8 h with continuous stirring. The mixture was then left at room temperature for 24 hs. A yellow precipitate was formed. The product was filtered, washed with warm ethanol, and crystallized from ethanol:dichloromethane solvent mixture (1 : 1). m.p. 190°C yield 60%; IR (KBr)ν(cm−1): 3296, 3203 (NH2); 3147 (NH-isatin); 1733 (C=O), 1614 (−C=N); 1540 (C–S + δNH, I); 1430 (C–N + C–S, II); 1197 (C–S, III); 835 (C=S, IV). 1H n.m.r. δ(ppm) (CD2Cl2)  12.012 (1H, s, NH); 7.653–6.94 (4H, m, aromatic); 2.022 (2H, d, NH2). MS, (m/z) (I%) (EI) calculated for C10H7N3OS2 m.wt 249 g/mole: 250 (10) [M+1]; 221 (3.2) [M–CO]; 207 (4) [M–NCO]; 162 (2); 119 (24); 90 (7.5).


## 3.2. 1-Morpholinomethyl-3-(1′-N-dithiooxamide)iminoisatin (LIH) and 1-diphenylaminomethyl-3-1′-N-dithiooxamide)Iminoisatin (LIIH)

(a) To a stirred solution of 3-(1′-N-dithiooxamide)iminoisatin (SBH) (0.01 mole, 2.49 g) and formaldehyde 37% (0.015 mole) in warm dry ethanol (20 mL) was added, drop by drop, (0.01 mole) of morpholine (LIH) or diphenylamine (LIIH). The mixture was heated under reflux for 3 h with continuous stirring, and then left to cool at room temperature. A solid precipitate was formed. The products were filtered, washed with warm ethanol, and then crystallized from ethanol : chloroform (1 : 1 v/v) mixture; yield 35 and 28.2%, respectively.(b) To a solution of dto (5 mmole, 0.6 g) in warm ethanol (10 mL) containing 2-3 drops glacial acetic acid was added (5 mmole) of Mannich base N-Morpholinomethylisatin (MI) or N-Diphenylaminomethyl isatin (MII) [16] in ethanol (10 mL) with continuous stirring, and the mixture was heated under reflux for 10 h. After leaving the mixture at room temperature for 24 h a precipitate was formed. The products were filtered, washed with warm ethanol, and crystallized; yield 20.3 and 21%, respectively (m.p. 215 and 283°C, resp.).1-Morpholinomethyle-3-(1′-N-dithiooxamide)iminoisa- tin (LIH):
yellowish orange crystals, m.p. 162°C; IR (KBr).ν(cm−1): 3203, 3138 (NH2); 3030–3000 (arom CH); 2815–2364 (CH2); 1730 (C=O); 1614 (−C=N); 1589 (C=C arom.); 1540 (νC=N, δNH, I); 1429 (C–N + C–S, II); 1195 (C–S, III); 835 (C=S, IV); 1149, 1328 (morpholine). 1H n.m.r δ(ppm) (DMSO): 7.59-6.898 (4H, m, aromatic +NH); 4.09 (2H, d, N–CH2N); 3.65 (4H, d, 2”, 6” CH2 morph.); 2.33 (4H, d, 3”, 5” CH2 morph.); 1.567 (1H, br, SH). MS (FAB) m/z (I%) calculated for C15H16N4O2S2, m.wt 348.45 g/mole,: 349.1 (93) [M]; 320 (38) [M–CO]; 235 (100); 234 (80); 220 (15), 207 (40). 131 (43); 104 (78%); (EI) m/z (I%): 348.5 (84) [M]; 320 (25) [M–CO]; 234 (38); 207 (17); 130 (19); 117 (24);  104 (57); 90 (30); 78 (22%). CHN% Calculated for C15H16N4O2S2 C, 51.67; H, 4.59, N, 16.07% found C, 50.69; H, 4.20; N, 15.75%; νmax (cm−1) (DMF) (εmax mol−1 cm−1) 34013 (20030) π→π*; 2415 (2980), n→π* (DMSO) 38461 (19519) π→π*.Diphenylaminomethyl-3-(1′-N-dithiooxamide)Iminoisa tin (LIIH):
yellow red crystals, m.p. 182, IR (KBr)ν(cm−1): 3193, 3034 (NH2); 1730 (C=O); 1614 (C=N); 1540, 1434, 1195, 833 (C–N + δNH, C–N + C–S, C–S, C=S I–IV, resp.). 1H n.m.r (δ, ppm) (CD2Cl2): 7.59–6.89 (14H, m, aromatic); 4.83 (2H, d, CH2); 2.17 (2H, b, NH2). MS m/z (I%) (EI): calculated for C23H18N4OS2, m.wt 430.55 g/mol: 430.9 (5.5) [M]; 402 (2.5) [M–CO]; 235 (21); 129.2 (1.8);  104 (4.8); 89 (10.3); 78.1 (3.5%). CHN (%) calculated for C23H18N4OS2: C, 64.18, H, 4.21; N, 13.02% found: C, 64.02; H, 4.22; N, 13.52%. νmax (cm−1) (DMF) (εmax, L mol−1 cm−1) 32258 (22970) π→π*; 24509 (3530) n→π*; (DMSO): 38461 (19540): 28571 (14120) π→π*.


## 4. Synthesis of Metal Complexes

To a solution of Schiff Mannich base ligand (2 mmole) in absolute ethanol (LIH) or ethanol and dimethylsulfoxide (1 : 1 v/v) (LIIH) (5 mL) was added an alcoholic solution (5 mL) of the metal salt (chlorides, nitrates, or acetates) (1 mmol), and the mixture was heated under reflux with continuous stirring for 3 h. Precipitation of products took place after heating time of 30 min for (Co(II)), Ni(II), and complexes of LIH and LIIH (C2, C3, C8, and C9, resp.), 1 h for (Mn(II), Cu(II), and Ir(III) complex of LIH and Cd(II) complex of LIIH (C1, C4, C5, and C12, resp.),  1.5 h for Pt(IV) complex of LIH (C7), 2 h for Pd(II) complex of LIH and Pt(IV) complex of LIIH (C6 and C11, resp.) and 3 h for Pd(II) complex of LIIH (C10). The products were filtered and purified from reactants  by washing many times with ethanol and ether (C1–C7) or with DMSO, ethanol and ether (C8–C12), and vacuum dried. Purity of the products was detected by TLC, using silica gel as a stationary phase and a mixture of chloroform and acetone (2 : 2 V/V) or various ratios of methyl acetate: acetone solvent mixture as eluents.


## 5. Biological Activity Study

### 5.1. Antibacterial Action

Antibacterial activities of the prepared compounds were tested against three types of pathogenic bacteria, namely,Escherichia coli, Staphylococcus  areus, and Proteus mirabilis using the antibiotic Ceftriaxone as a control. Bacterial cultures were prepared by streaking (0.1) mL of 106 CFU/mL broth of indicator strain on the whole surface of nutrient agar plate. In each plate four wells (pores) were created on the nutrient agar layer using sterile cork porer. In each hole was injected 50 μL of 10−3 M of the studied compounds in DMSO by micropipette. The resulting cultures were incubated at 37°C for 24 h. The inhibition zones caused by each compound were measured, and the results were interpreted according to diameter measurements.


### 5.2. Cytotoxic Activity

A preliminary study of cytotoxic activity of some of the prepared compounds was performed against human epidermoid larynx carcinoma cell lines (Hep-2) of 52-year-old patient. Hep-2 monolayer cell lines were prepared by subculturing cell line into (RPMI-1640) medium supplemented with 10% heat deactivated fetal bovine serum. The resulting media were incubated at 37°C for 48 h until confluent layer was achieved. Four concentrations of investigated compounds were prepared: 62.5, 125, 250, and 500μg/mL using dimethyl sulfoxide (DMSO) as a diluent. Hep-2 cell line was plated into 96-well microtiter plates. Then 0.2 mL of each tested compound was added to each well in triplicates, and incubation was carried out for 48 h. Cultures were stained with 50 μL/well Neutral Red (NR) solution. The stained cultures were left in the incubator for further 2 h, washed with phosphate buffered saline solution followed by (0.1 mL) ethanol phosphate buffered solution (NaH2PO4 : ethanol (1 : 1), vehicle ethanol). The cytotoxic effects of the applied compounds were measured in terms of optical density of viable cells at λ=492 nm using a Micro ELISA reader.


## 5.1. Antibacterial Action

Antibacterial activities of the prepared compounds were tested against three types of pathogenic bacteria, namely,Escherichia coli, Staphylococcus  areus, and Proteus mirabilis using the antibiotic Ceftriaxone as a control. Bacterial cultures were prepared by streaking (0.1) mL of 106 CFU/mL broth of indicator strain on the whole surface of nutrient agar plate. In each plate four wells (pores) were created on the nutrient agar layer using sterile cork porer. In each hole was injected 50 μL of 10−3 M of the studied compounds in DMSO by micropipette. The resulting cultures were incubated at 37°C for 24 h. The inhibition zones caused by each compound were measured, and the results were interpreted according to diameter measurements.


## 5.2. Cytotoxic Activity

A preliminary study of cytotoxic activity of some of the prepared compounds was performed against human epidermoid larynx carcinoma cell lines (Hep-2) of 52-year-old patient. Hep-2 monolayer cell lines were prepared by subculturing cell line into (RPMI-1640) medium supplemented with 10% heat deactivated fetal bovine serum. The resulting media were incubated at 37°C for 48 h until confluent layer was achieved. Four concentrations of investigated compounds were prepared: 62.5, 125, 250, and 500μg/mL using dimethyl sulfoxide (DMSO) as a diluent. Hep-2 cell line was plated into 96-well microtiter plates. Then 0.2 mL of each tested compound was added to each well in triplicates, and incubation was carried out for 48 h. Cultures were stained with 50 μL/well Neutral Red (NR) solution. The stained cultures were left in the incubator for further 2 h, washed with phosphate buffered saline solution followed by (0.1 mL) ethanol phosphate buffered solution (NaH2PO4 : ethanol (1 : 1), vehicle ethanol). The cytotoxic effects of the applied compounds were measured in terms of optical density of viable cells at λ=492 nm using a Micro ELISA reader.


## 6. Results and Discussions

### 6.1. Synthesis

The synthesis of the two new ligands has been achieved by following two different pathways A and B as is illustrated by Scheme2. Pathway A involves the synthesis of Schiff base precursor of  isatin (SBH) followed by condensation with the secondary amine,  morpholine or diphenylamine, in presence of formaldehyde to form LIH and LIIH, respectively.  Pathway B involves the formation of Mannich base precursor of isatin (MI and MII) followed by condensation reaction with dithiooxamide. The second method showed lower yield and longer reaction time.Scheme 2
Synthesis of Schiff Mannich base ligands from isatin and dithiooxamide.The1H n.m.r spectrum of the Schiff base precursor SBH in CD2Cl2 (Figure 1) is characterized by the appearance of chemical shift related to the NH2 protons of dto moiety at δ2.022 ppm [11, 20, 21] and the appearance of NH proton of isatin ring at δ12.012 ppm [5–7, 22–25] which is quite agreeable with the suggested structure of SBH. The 1H n.m.r spectrum of LIIH in CD2Cl2 exhibited chemical shifts of NH2 protons at 2.17 ppm while that of LIH in DMSO (Figure 2) gave chemical shifts at δ1.567 ppm. This was attributed to tautomerism of LIH in DMSO to iminosulfhydryl structure in equilibrium with dithioamide structure, as a result of solvent polarity [26, 27]. Such behavior was confirmed by the appearance of the signal assigned to imino NH group at lower field. The spectrum of LIIH (Figure 3) exhibited chemical shifts of aromatic protons of isatin ring and diphenylamine at δ6.89–7.11 and at δ7.68–7.59, respectively, while those of methylene group appeared at high fields [22–24].Figure 1
1HNMR Spectrum of SBH in CD2Cl2.Figure 2
1HNMR Spectrum of LIH in DMSO.Figure 3
1HNMR of  LIIH  spectrum  in CD2Cl2.The mass spectra of the two Mannich and Schiff base ligands as well as SBH are shown in Figures4, 5, and 6, respectively. The EI mode of mass spectrum displayed by SBH (Figure 6) gave a peak at m/z = 250 which was assigned to [M+1], while the two Mannich base ligands displayed peaks corresponding to [M+] molecular ions. Smaller fragments were also observed and were characteristic of isatin behavior of other compounds [1, 22, 26, 28–34]. The FAB and EI modes of LIH (Figures 4(a) and 4(b)) showed different intensities of common fragments ions.Mass spectrum of LIH by (a)  FAB and (b) EI modes.
(a)(b)Figure 5
Mass spectrum of LIIH.Figure 6
Mass spectrum of SBH.The IR spectra of the three organic compounds exhibited the disappearance of stretching modes assigned to C-3 carbonyl of isatin ring and appearance of stretching modes of azomethine group of Schiff base products at 1614 cm−1   [35]. Stretching vibrations of C-2 carbonyl group of isatin ring for SBH and the two Mannich Schiff base ligands were observed at 1733–1730 cm−1  [35]. The presence of bands assigned to NH2 asymmetric symmetric stretching vibrations indicates that the formation of Schiff bases was through one NH2 group only. Both ligands exhibited the absence of stretching vibrations assigned to NH of isatin ring, and instead vibrational modes of N–CH2 groups were observed at 2813–2304 cm−1   [35]. Bands observed at 1149, 1328 in the spectrum of LIH were attributed to C–O–C and C–N–C vibration of morpholine ring, respectively [35–38].


### 6.2. Physical Properties and Analytical Data of Metal Complexes

The color, melting points, yields, and elemental analyses of the prepared metal complexes of isatin Schiff Mannich base ligands are described in Table1. Most results were in agreement with the suggested formula. Some deviations in elemental analyses may be attributed to incomplete combustion of the complexes. The low yield resulted from extensive purification of products from the starting materials as was indicated from TLC results.Table 1
Physical properties and analytical data of the prepared  Schiff   and  Mannich  base   complexes.
Molecular formula(Color)m.p. (decomposition) temp. °CYield %% element analysis found (calculated)CHNMCl[Mn(LIH)(H2O)Cl2] 2.5H2O (Brown) (C1)21542.2433.91(33.46)4.22(4.27)11.18(10.40)10.66(10.20)13.11(13.19)[Co(LIH)(NO3)2]H2O (Brown) (C2)17461.1133.11(32.77)3.02(3.27)16.09(15.29)10.50(10.73)—[Ni(LIH)2]2NO3·H2O (Bright blue) (C3)>30050.840.90(40.13)3.62(3.78)16.06(15.60)5.78(6.54)—[Cu2(LIH)2Cl(H2O)4]Cl3  (Reddish brown) (C4)>30077.1140.25(39.85)4.32(4.43)6.81(6.20)13.73(14.07)7.26(7.86)[PdLI]Cl·1.5H2O (Dark brown) (C5)25059.2134.45(34.82)3.01(3.48)11.32(10.80)—7.01(6.86)[Ir(LIH)2Cl2]Cl·H2O (Pale yellow) (C6)23032.3134.73(35.51)3.32(3.55)11.82(11.05)19.56(19.12)9.98(10.50)[Pt(LI)Cl3]0.5H2O (Yellow brown) (C7)>30034.0127.78(27.31)2.49(2.58)8.82(8.49)28.89(29.60)16.82(16.16)[Co2(LIIH)2(NO3)4]·2H2O (Dark green) (C8)23542.1544.62(43.74)3.71(3.17)13.64(13.31)8.89(9.34)—[Ni(LIIH)(OAc)2] (Blue) (C9)24350.3252.84(53.40)3.54(3.95)9.43(9.23)9.72(9.23)—[PdLIICl]21.5H2O (Dark brown) (C10)>28023.3046.51(46.86)3.81(3.23)10.11(9.51)—6.40(6.03)[Pt(LII)Cl2·H2O]Cl·H2O (Brown) (C11)25033.2336.21(35.95)2.13(2.87)8.23(7.29)24.77(25.40)13.09(13.87)[CdLII (OAc)(H2O)2]2 (Yellow) (C12)26020.5746.65(47.06)3.62(3.29)9.50(8.77)16.95(17.63)—


### 6.3. Infrared Spectra

The important stretching vibrations of LIH and LIIH metal complexes are described in Table 2. The Mn(II), Co(II) and Ni(II) complexes of LIH (C1–C3, resp.) and Co(II) complex of LIIH (C8) exhibited shifts of the thioamide groups to lower frequencies indicating the involvement of thiocarbonyl sulfur atoms in coordination with these metal ions [39, 40]. The spectra of C1 and C2 demonstrated further shift of NH2 group vibrational modes to lower frequencies as a result of bonding. On the other hand the spectra of Cu(II), Ir(III), and Pt(IV) complexes of LIH (C4, C6, C7, resp.) and Pd(II), Pt(IV), and Cd(II) complexes of LIIH (C10–C12, resp.) displayed the disappearance of the stretching mode of thioamide NH2 group and the shift of C-S band to lower frequencies. This refers to the bonding of metal ion to the deprotonated group of the ligand in the form of  as in C4, C6, and C9 or in the form of  anion as in the case of C5, C7, and C10–C12. The appearance of stretching modes assigned to NH and C=N of −C=NH groups was observed at 3371–3100 and 1640–1620 cm−1, respectively [15, 35, 39, 41]. The stretching vibrations of azomethine group of the Schiff base ligands were shifted to lower frequencies in all spectra except those of C6, C10, and C12, whereas stretching vibrations of carbonyl group were shifted to lower frequencies in all spectra except C1, C4, C6, and C10 indicating additional coordination of metal ions to C=N and C=O groups [36–38]. Bands related to coordinated water vibrations were observed in the spectra of C1, C4, and C12 at (3490, 756, 640), (3480, 800, 730), and (3500, 864, 710) cm−1, respectively, and to lattice water vibrations at frequency range 3519–3464 cm−1 in the other complexes. The bands related to nitrate ions were observed in the spectra of C2and C3 at (1522, 1478), (1765, 1641) cm−1 and were assigned to monodentate and free ion behaviors, respectively, whereas that of C8appeared at 1750–1660 and 1406–1380 cm−1 showing monodentate and bidentate behaviors, respectively [42]. Bands attributed to acetate group vibrations were observed in the spectra of C9 and C12 at (1645, 1340) and (1590, 1465) cm−1, respectively, indicating monodentate and bidentate bridging behaviors, respectively [42]. Additional bands were observed at lower frequencies (600–250 cm−1) and were attributed to M–N, M–O, M–S, and M–X (X = acetate, NO3−, Cl−) stretching modes [42].Table 2
Important  I.R. vibrations (cm−1) for  the two Mannich and Schiff base ligands and their metal complexes.
SymbolνNH2νC=OνC=NThioamide groupνM-NνM-OνM-SνM-ClBand (I)δN-H +   νC-SBand  (II)νC-N +νC-SBand        (III)νC-SBand (IV)νC=SLIH3138—1730–17351614154014291195835————3203C1Mn(II)3124—17321600151014341190820248283325246a3371C2Co(II)3072—17241602153014331163777230460330—3263270C3Ni(II)3133—17201595153514271150827293464330—3213C4Cu(II)—331517351600153514341190792250457350222b1650302C5Pd(II)—339217081604153714301190815240459323—1660301C6Ir(III)—334217351614153914001151810350—330253a1650C7Pt(IV)—316817001600151714461114833254462329297a1650LIIH3043—17301614154014341195833————3193C8Co(II)3151—17001602158514401130800393400327—3321227C9Ni(II)3128324916951600158314841150809246478320—3249250340C10Pd(II)—342517351619158714501155820464—323240b32491647210C11Pt(IV)—323017301616153014301150802468450325291a1650480262C12Cd(II)—330017351616148814301161800288468325—1650450a: terminal; b: bridging.


### 6.4. Thermal Analysis

Steps of thermal decomposition of the Co(II) and Ir(III) complexes of LIH (C2, C6) following TG and DTG curves under nitrogen atmosphere and heating range 50–800°C are described in Table 3, and their thermographs are shown in Figures 7 and 8, respectively. At low temperatures, the initial weight losses were determined from TG curves referred to loss of water of crystallization [43–45]. The final stage of thermal decomposition of C2 gave the metal oxide whereas the Ir complex (C6) gave the free metal as a final residue [43–45].Table 3
Suggested   thermal decomposition  steps of C2 and C6.
Stable phase (M.wt)[CoLI (NO3)2]·H2O (C2) (549.193)Temp. range of decomp. at TG °CPeak temp. at DTG °C%weight loss found (calc.)H2O (Lattice)70–120—2.91(3.27)NO3120–22020011.62(11.97)C15N4H16O2S2  NO2220–600—71.38(71.80)CoO——13.28(13.64)[Ir(LI)2Cl2]Cl·(0.5)H2O (C6)(1004.24)0.5H2O (lattice)  C8N2H16O280–25019017.43(17.62)3Cl  C9N2H8250–50039924.07(24.94)C10N3H6OS2500–70051524.48(24.69)C2NS2H2700–83076013.30(13.14)Ir——19.83(19.12)Figure 7
Thermographs of  the  Co(II) complex of LIH (C2).Figure 8
Thermographs of  the Ir(III)complex of LIH (C6).


### 6.5. Electronic Spectra and Suggested Structures

Table4 describes the energies of bands observed in the spectra of metal complexes and their assignments together with magnetic moments and molar conductivity in DMF (10−3 M). The spectral parameters 10 Dq, Dq/B¯, B¯, and β as well as energies of unobserved ligand field bands were obtained by applying observed band energies and band ratios on Tanabe-Saugano diagrams of the specified metal ion [46–48]. All metal complexes exhibited spectra related to octahedral arrangement of ligand atoms around the metal ions except those of palladium(II) as they gave square planar geometries. The high values of magnetic moments of Co(II), Ni(II), and Cu(II) complexes are attributed to spin-orbital coupling [49]. All complexes were of high-spin octahedral geometries except Pt(IV), Ir(III), and Cd(II) complexes which were diamagnetic and so were Pd(II) complexes.Table 4
Electronic spectra, spectral parameters, molar conductivity, and  effective magnetic moments (μeff) of Schiff  and Mannich base complexes.
Comp. no.Band  positions (cm-1)AssignmentDq/B/(B/)(cm-1)β10Dq (cm-1)Ω (S.mol-.cm2)μeff  (BM)C1 Mn(II)ν1178576A1g(S)→4T2g(G)———15.05.851ν2  25641L → M (C.T.)C2 Co(II)ν1  5352(*)4T1g →4T2g0963(705)0.72667896.055.446ν2  133334T1g (F) →4A2gν3  166254T1g(F)→4T1g (P)ν4   27777L → M (C.T.)C3 Ni(II)ν1  102043A2g →3T2g31.65(619.6)0.60210223186.04.18ν2  14388A2g →3T1g (F)3ν3  21276A2g →3T1g (P)C4Cu(II)ν1  111112B1g →2A1g———282.02.51ν2  166672B1g →2B2gν3  222222B1g →2Egν4  28571L → M (C.T.)C5Pd(II)ν1  163931A1g →1A2g———77.0Diamag.ν2  212761A1g →1B1gC6Ir(III)ν1  147051A1g →3T1g———90.0Diamag.ν2  185181A1g →1T2gν3  22222L → M (C.T.)C7Pt(IV)ν1  156251A1g →3T1g———15.0Diamag.ν2  212761A1g →3T2gν3  23255L → M (C.T.)C8Co(II)ν1  5471(*)4T1g →4T2g0.843 (762.61)0785643018.04.617ν2  109894T1g →4A2gν3  157954T1g (F) →4T1g (P)ν4   26315L → M (C.T.)C9Ni(II)ν1  101723A2g →3T2g1.667 (612.2)05941020020.54.251ν2  148453A2g →3T1g (F)ν3  227273A1g →3T1g (P)ν4  27027L → M (C.T.)C10Pd(II)ν1  160251A1g →1A2g———9.0Diamag.ν2  217391A1g →1B1gν3  263151A1g →1EgC11 Pt(IV)ν1  159081A1g →3T1g———73.0Diamag.ν2  27027L → M (C.T.)C12 Cd(II)ν1  27777L → M (C.T.)8.00Diamag.ν2  32786Intraligπ→π**  Calculated.The spectrum of the Cd(II) complex (C12) exhibited charge transfer bands only, which is a common phenomenon for d10 metal complexes where d-d transitions are excluded [47, 48]. Conductivity measurement of metal complexes in DMF solution (10−3 M) showed nonelectrolytic nature of Mn(II), Co(II), and Pt(IV) complexes of LIH (C1, C2, and C7, resp.) and Co(II), Ni(II), Pd(II), and Cd(II) complexes of LIIH (C8–C10 and C12, resp.) [50]. Electrolytic nature of 1 : 1 was exhibited by Pd(II), Ir(III) complexes of LIH (C5 and C6) and Pt(IV) complex of LIIH (C11), 1 : 2 by Ni(II) complex of LIH (C3) and 1 : 3 by Cu(II) complex of LIH (C4) [50]. According to the above-mentioned data and those of elemental analyses and i.r. spectra, the structures of the metal complexes can be suggested as illustrated in Scheme 3.Suggested structures of Schiff and Mannich base complexes.


## 6.1. Synthesis

The synthesis of the two new ligands has been achieved by following two different pathways A and B as is illustrated by Scheme2. Pathway A involves the synthesis of Schiff base precursor of  isatin (SBH) followed by condensation with the secondary amine,  morpholine or diphenylamine, in presence of formaldehyde to form LIH and LIIH, respectively.  Pathway B involves the formation of Mannich base precursor of isatin (MI and MII) followed by condensation reaction with dithiooxamide. The second method showed lower yield and longer reaction time.Scheme 2
Synthesis of Schiff Mannich base ligands from isatin and dithiooxamide.The1H n.m.r spectrum of the Schiff base precursor SBH in CD2Cl2 (Figure 1) is characterized by the appearance of chemical shift related to the NH2 protons of dto moiety at δ2.022 ppm [11, 20, 21] and the appearance of NH proton of isatin ring at δ12.012 ppm [5–7, 22–25] which is quite agreeable with the suggested structure of SBH. The 1H n.m.r spectrum of LIIH in CD2Cl2 exhibited chemical shifts of NH2 protons at 2.17 ppm while that of LIH in DMSO (Figure 2) gave chemical shifts at δ1.567 ppm. This was attributed to tautomerism of LIH in DMSO to iminosulfhydryl structure in equilibrium with dithioamide structure, as a result of solvent polarity [26, 27]. Such behavior was confirmed by the appearance of the signal assigned to imino NH group at lower field. The spectrum of LIIH (Figure 3) exhibited chemical shifts of aromatic protons of isatin ring and diphenylamine at δ6.89–7.11 and at δ7.68–7.59, respectively, while those of methylene group appeared at high fields [22–24].Figure 1
1HNMR Spectrum of SBH in CD2Cl2.Figure 2
1HNMR Spectrum of LIH in DMSO.Figure 3
1HNMR of  LIIH  spectrum  in CD2Cl2.The mass spectra of the two Mannich and Schiff base ligands as well as SBH are shown in Figures4, 5, and 6, respectively. The EI mode of mass spectrum displayed by SBH (Figure 6) gave a peak at m/z = 250 which was assigned to [M+1], while the two Mannich base ligands displayed peaks corresponding to [M+] molecular ions. Smaller fragments were also observed and were characteristic of isatin behavior of other compounds [1, 22, 26, 28–34]. The FAB and EI modes of LIH (Figures 4(a) and 4(b)) showed different intensities of common fragments ions.Mass spectrum of LIH by (a)  FAB and (b) EI modes.
(a)(b)Figure 5
Mass spectrum of LIIH.Figure 6
Mass spectrum of SBH.The IR spectra of the three organic compounds exhibited the disappearance of stretching modes assigned to C-3 carbonyl of isatin ring and appearance of stretching modes of azomethine group of Schiff base products at 1614 cm−1   [35]. Stretching vibrations of C-2 carbonyl group of isatin ring for SBH and the two Mannich Schiff base ligands were observed at 1733–1730 cm−1  [35]. The presence of bands assigned to NH2 asymmetric symmetric stretching vibrations indicates that the formation of Schiff bases was through one NH2 group only. Both ligands exhibited the absence of stretching vibrations assigned to NH of isatin ring, and instead vibrational modes of N–CH2 groups were observed at 2813–2304 cm−1   [35]. Bands observed at 1149, 1328 in the spectrum of LIH were attributed to C–O–C and C–N–C vibration of morpholine ring, respectively [35–38].


## 6.2. Physical Properties and Analytical Data of Metal Complexes

The color, melting points, yields, and elemental analyses of the prepared metal complexes of isatin Schiff Mannich base ligands are described in Table1. Most results were in agreement with the suggested formula. Some deviations in elemental analyses may be attributed to incomplete combustion of the complexes. The low yield resulted from extensive purification of products from the starting materials as was indicated from TLC results.Table 1
Physical properties and analytical data of the prepared  Schiff   and  Mannich  base   complexes.
Molecular formula(Color)m.p. (decomposition) temp. °CYield %% element analysis found (calculated)CHNMCl[Mn(LIH)(H2O)Cl2] 2.5H2O (Brown) (C1)21542.2433.91(33.46)4.22(4.27)11.18(10.40)10.66(10.20)13.11(13.19)[Co(LIH)(NO3)2]H2O (Brown) (C2)17461.1133.11(32.77)3.02(3.27)16.09(15.29)10.50(10.73)—[Ni(LIH)2]2NO3·H2O (Bright blue) (C3)>30050.840.90(40.13)3.62(3.78)16.06(15.60)5.78(6.54)—[Cu2(LIH)2Cl(H2O)4]Cl3  (Reddish brown) (C4)>30077.1140.25(39.85)4.32(4.43)6.81(6.20)13.73(14.07)7.26(7.86)[PdLI]Cl·1.5H2O (Dark brown) (C5)25059.2134.45(34.82)3.01(3.48)11.32(10.80)—7.01(6.86)[Ir(LIH)2Cl2]Cl·H2O (Pale yellow) (C6)23032.3134.73(35.51)3.32(3.55)11.82(11.05)19.56(19.12)9.98(10.50)[Pt(LI)Cl3]0.5H2O (Yellow brown) (C7)>30034.0127.78(27.31)2.49(2.58)8.82(8.49)28.89(29.60)16.82(16.16)[Co2(LIIH)2(NO3)4]·2H2O (Dark green) (C8)23542.1544.62(43.74)3.71(3.17)13.64(13.31)8.89(9.34)—[Ni(LIIH)(OAc)2] (Blue) (C9)24350.3252.84(53.40)3.54(3.95)9.43(9.23)9.72(9.23)—[PdLIICl]21.5H2O (Dark brown) (C10)>28023.3046.51(46.86)3.81(3.23)10.11(9.51)—6.40(6.03)[Pt(LII)Cl2·H2O]Cl·H2O (Brown) (C11)25033.2336.21(35.95)2.13(2.87)8.23(7.29)24.77(25.40)13.09(13.87)[CdLII (OAc)(H2O)2]2 (Yellow) (C12)26020.5746.65(47.06)3.62(3.29)9.50(8.77)16.95(17.63)—


## 6.3. Infrared Spectra

The important stretching vibrations of LIH and LIIH metal complexes are described in Table 2. The Mn(II), Co(II) and Ni(II) complexes of LIH (C1–C3, resp.) and Co(II) complex of LIIH (C8) exhibited shifts of the thioamide groups to lower frequencies indicating the involvement of thiocarbonyl sulfur atoms in coordination with these metal ions [39, 40]. The spectra of C1 and C2 demonstrated further shift of NH2 group vibrational modes to lower frequencies as a result of bonding. On the other hand the spectra of Cu(II), Ir(III), and Pt(IV) complexes of LIH (C4, C6, C7, resp.) and Pd(II), Pt(IV), and Cd(II) complexes of LIIH (C10–C12, resp.) displayed the disappearance of the stretching mode of thioamide NH2 group and the shift of C-S band to lower frequencies. This refers to the bonding of metal ion to the deprotonated group of the ligand in the form of  as in C4, C6, and C9 or in the form of  anion as in the case of C5, C7, and C10–C12. The appearance of stretching modes assigned to NH and C=N of −C=NH groups was observed at 3371–3100 and 1640–1620 cm−1, respectively [15, 35, 39, 41]. The stretching vibrations of azomethine group of the Schiff base ligands were shifted to lower frequencies in all spectra except those of C6, C10, and C12, whereas stretching vibrations of carbonyl group were shifted to lower frequencies in all spectra except C1, C4, C6, and C10 indicating additional coordination of metal ions to C=N and C=O groups [36–38]. Bands related to coordinated water vibrations were observed in the spectra of C1, C4, and C12 at (3490, 756, 640), (3480, 800, 730), and (3500, 864, 710) cm−1, respectively, and to lattice water vibrations at frequency range 3519–3464 cm−1 in the other complexes. The bands related to nitrate ions were observed in the spectra of C2and C3 at (1522, 1478), (1765, 1641) cm−1 and were assigned to monodentate and free ion behaviors, respectively, whereas that of C8appeared at 1750–1660 and 1406–1380 cm−1 showing monodentate and bidentate behaviors, respectively [42]. Bands attributed to acetate group vibrations were observed in the spectra of C9 and C12 at (1645, 1340) and (1590, 1465) cm−1, respectively, indicating monodentate and bidentate bridging behaviors, respectively [42]. Additional bands were observed at lower frequencies (600–250 cm−1) and were attributed to M–N, M–O, M–S, and M–X (X = acetate, NO3−, Cl−) stretching modes [42].Table 2
Important  I.R. vibrations (cm−1) for  the two Mannich and Schiff base ligands and their metal complexes.
SymbolνNH2νC=OνC=NThioamide groupνM-NνM-OνM-SνM-ClBand (I)δN-H +   νC-SBand  (II)νC-N +νC-SBand        (III)νC-SBand (IV)νC=SLIH3138—1730–17351614154014291195835————3203C1Mn(II)3124—17321600151014341190820248283325246a3371C2Co(II)3072—17241602153014331163777230460330—3263270C3Ni(II)3133—17201595153514271150827293464330—3213C4Cu(II)—331517351600153514341190792250457350222b1650302C5Pd(II)—339217081604153714301190815240459323—1660301C6Ir(III)—334217351614153914001151810350—330253a1650C7Pt(IV)—316817001600151714461114833254462329297a1650LIIH3043—17301614154014341195833————3193C8Co(II)3151—17001602158514401130800393400327—3321227C9Ni(II)3128324916951600158314841150809246478320—3249250340C10Pd(II)—342517351619158714501155820464—323240b32491647210C11Pt(IV)—323017301616153014301150802468450325291a1650480262C12Cd(II)—330017351616148814301161800288468325—1650450a: terminal; b: bridging.


## 6.4. Thermal Analysis

Steps of thermal decomposition of the Co(II) and Ir(III) complexes of LIH (C2, C6) following TG and DTG curves under nitrogen atmosphere and heating range 50–800°C are described in Table 3, and their thermographs are shown in Figures 7 and 8, respectively. At low temperatures, the initial weight losses were determined from TG curves referred to loss of water of crystallization [43–45]. The final stage of thermal decomposition of C2 gave the metal oxide whereas the Ir complex (C6) gave the free metal as a final residue [43–45].Table 3
Suggested   thermal decomposition  steps of C2 and C6.
Stable phase (M.wt)[CoLI (NO3)2]·H2O (C2) (549.193)Temp. range of decomp. at TG °CPeak temp. at DTG °C%weight loss found (calc.)H2O (Lattice)70–120—2.91(3.27)NO3120–22020011.62(11.97)C15N4H16O2S2  NO2220–600—71.38(71.80)CoO——13.28(13.64)[Ir(LI)2Cl2]Cl·(0.5)H2O (C6)(1004.24)0.5H2O (lattice)  C8N2H16O280–25019017.43(17.62)3Cl  C9N2H8250–50039924.07(24.94)C10N3H6OS2500–70051524.48(24.69)C2NS2H2700–83076013.30(13.14)Ir——19.83(19.12)Figure 7
Thermographs of  the  Co(II) complex of LIH (C2).Figure 8
Thermographs of  the Ir(III)complex of LIH (C6).


## 6.5. Electronic Spectra and Suggested Structures

Table4 describes the energies of bands observed in the spectra of metal complexes and their assignments together with magnetic moments and molar conductivity in DMF (10−3 M). The spectral parameters 10 Dq, Dq/B¯, B¯, and β as well as energies of unobserved ligand field bands were obtained by applying observed band energies and band ratios on Tanabe-Saugano diagrams of the specified metal ion [46–48]. All metal complexes exhibited spectra related to octahedral arrangement of ligand atoms around the metal ions except those of palladium(II) as they gave square planar geometries. The high values of magnetic moments of Co(II), Ni(II), and Cu(II) complexes are attributed to spin-orbital coupling [49]. All complexes were of high-spin octahedral geometries except Pt(IV), Ir(III), and Cd(II) complexes which were diamagnetic and so were Pd(II) complexes.Table 4
Electronic spectra, spectral parameters, molar conductivity, and  effective magnetic moments (μeff) of Schiff  and Mannich base complexes.
Comp. no.Band  positions (cm-1)AssignmentDq/B/(B/)(cm-1)β10Dq (cm-1)Ω (S.mol-.cm2)μeff  (BM)C1 Mn(II)ν1178576A1g(S)→4T2g(G)———15.05.851ν2  25641L → M (C.T.)C2 Co(II)ν1  5352(*)4T1g →4T2g0963(705)0.72667896.055.446ν2  133334T1g (F) →4A2gν3  166254T1g(F)→4T1g (P)ν4   27777L → M (C.T.)C3 Ni(II)ν1  102043A2g →3T2g31.65(619.6)0.60210223186.04.18ν2  14388A2g →3T1g (F)3ν3  21276A2g →3T1g (P)C4Cu(II)ν1  111112B1g →2A1g———282.02.51ν2  166672B1g →2B2gν3  222222B1g →2Egν4  28571L → M (C.T.)C5Pd(II)ν1  163931A1g →1A2g———77.0Diamag.ν2  212761A1g →1B1gC6Ir(III)ν1  147051A1g →3T1g———90.0Diamag.ν2  185181A1g →1T2gν3  22222L → M (C.T.)C7Pt(IV)ν1  156251A1g →3T1g———15.0Diamag.ν2  212761A1g →3T2gν3  23255L → M (C.T.)C8Co(II)ν1  5471(*)4T1g →4T2g0.843 (762.61)0785643018.04.617ν2  109894T1g →4A2gν3  157954T1g (F) →4T1g (P)ν4   26315L → M (C.T.)C9Ni(II)ν1  101723A2g →3T2g1.667 (612.2)05941020020.54.251ν2  148453A2g →3T1g (F)ν3  227273A1g →3T1g (P)ν4  27027L → M (C.T.)C10Pd(II)ν1  160251A1g →1A2g———9.0Diamag.ν2  217391A1g →1B1gν3  263151A1g →1EgC11 Pt(IV)ν1  159081A1g →3T1g———73.0Diamag.ν2  27027L → M (C.T.)C12 Cd(II)ν1  27777L → M (C.T.)8.00Diamag.ν2  32786Intraligπ→π**  Calculated.The spectrum of the Cd(II) complex (C12) exhibited charge transfer bands only, which is a common phenomenon for d10 metal complexes where d-d transitions are excluded [47, 48]. Conductivity measurement of metal complexes in DMF solution (10−3 M) showed nonelectrolytic nature of Mn(II), Co(II), and Pt(IV) complexes of LIH (C1, C2, and C7, resp.) and Co(II), Ni(II), Pd(II), and Cd(II) complexes of LIIH (C8–C10 and C12, resp.) [50]. Electrolytic nature of 1 : 1 was exhibited by Pd(II), Ir(III) complexes of LIH (C5 and C6) and Pt(IV) complex of LIIH (C11), 1 : 2 by Ni(II) complex of LIH (C3) and 1 : 3 by Cu(II) complex of LIH (C4) [50]. According to the above-mentioned data and those of elemental analyses and i.r. spectra, the structures of the metal complexes can be suggested as illustrated in Scheme 3.Suggested structures of Schiff and Mannich base complexes.


## 7. Biological Activity

### 7.1. Antibacterial Activity

The growth inhibition of the prepared Schiff and Mannich base ligands and some selected metal complexes were studied against three types of pathogenic bacteria, namely,Proteus mirabilis, Escherichia coli, and Staphylococcus aureus by using DMSO as a solvent and the antibiotic  Ceftriaxone as a control. Cultures were incubated at 37°C for 24 h. The inhibition zones were measured, and results are described in Table 5. The Schiff base precursor (SBH) and LIH were potent against all types of bacteria with the latter being more active than Ceftriaxone, while LIIH was inactive. Complexes of LIH with Co(II), Ni(II), Pd(II), and Ir(III) ions (C2, C3, C5, C6) showed no activity while the Pt(IV) complex (C7) was as active as the original ligand against all types. Among the selected metal complexes of LIIH, the Pd(II) complex (C10) was highly potent against all bacterial cultures. These results indicate that the degree of growth inhibition is highly dependent on the structure of ligands, metal complexes, and type of metal ion [51, 52]. Although the inhibition zones of LIH, C7 and C10  were larger than that caused by Ceftriaxone, other categories, like toxicity of these compounds, still have to be studied in detail.Table 5
Antibacterial activities of the Schiff and Mannich bases and  some selected metal complexes showing inhibition zones in diameters (mm).
EntryCompoundProteus mirabilisEscherichia coliStaphylococcus aureus1SBH19++30+++29+++2LIH32++++48+++++43+++++3Co(II) (C2)——————4Pd(II) (C5)——8—9—5Ir(III) (C6)——10—9—6Pt(IV) (C7)38+++++39+++++44+++++7LIIH9—9—12—8Co(II) (C8)9—8—15+9Pd(II) (C10)38+++++39+++++44+++++10Cd(II) (C12)9—8—15+11ceftriaxone28+++30+++36++++


### 7.2. Cytotoxic Effect

Preliminary cytotoxicity tests of the Schiff base (SBH) and its Mannich base ligands (LIH and LIIH) with some selected metal complexes were performed in triplicate against cancer cell line of human epidermoid larynx carcinoma (Hep-2) using concentrations of 62.5, 125, 250, and 500 μg/mL in DMSO with exposure time of 48 h using ELISA spectrophotometer. The three organic compounds showed high toxic activities at 125, 250, 250 μg/mL, respectively, causing cell death as was confirmed by the drop in optical absorbance of NR in the treated cells compared with the controls which refers to complete disruption of cell functions [53]. The cytotoxic effect of metal complexes of LIH was found to increase in the order of Pt(IV) < Pd(II) << Ir(III) as is shown in Figure 9. The Pt(IV) complex (C7) was much less active than the parent ligand, and its performance was found to decrease with concentration that it was totally inactive at 500 μg/mL.Cytotoxic effect of LIH, LIIH, and some selected metal complexes on growth of cancer cell line Hep-2 at different concentrations with exposure time 48 h.
(a)(b)The Pd(II) complex (C5) followed the same trend of concentration as the Pt(IV) complex but it was toxic enough to cause cell death. The Ir(III) complex (C6) was exceptionally active, and its cytotoxic activity was found to increase with concentration. Figure 10 illustrates the difference in dye distribution in the tissue culture sections of Hep-2 before and after treatment with this complex in comparison with the control. Both the Pd(II) and Cd(II) complexes of LIIH (C10 and C12) were less toxic than the parent ligand, and their activity slightly increased with concentration. The Cd(II) complex (C12) caused 30–60% decrease of ligand activity. The complex was similarly inactive against growth of the three bacterial cultures although Cd++ ion is well known as an environmental carcinogen at very low concentrations in human and animals [54]. This indicates that the toxicity of Cd++ ion can be decreased on complexation with some ligands.Tissue culture sections of Hep-2 cell line before (c) and after treatment with IrLI (C6).
(a)(b)The present study describes a narrow scope of the cytotoxic activity of the studied compounds.  Extension of this study, in future work to involve other cancer cell lines and other metal complexes, using normal human cell lines as control, may reveal more important data.


## 7.1. Antibacterial Activity

The growth inhibition of the prepared Schiff and Mannich base ligands and some selected metal complexes were studied against three types of pathogenic bacteria, namely,Proteus mirabilis, Escherichia coli, and Staphylococcus aureus by using DMSO as a solvent and the antibiotic  Ceftriaxone as a control. Cultures were incubated at 37°C for 24 h. The inhibition zones were measured, and results are described in Table 5. The Schiff base precursor (SBH) and LIH were potent against all types of bacteria with the latter being more active than Ceftriaxone, while LIIH was inactive. Complexes of LIH with Co(II), Ni(II), Pd(II), and Ir(III) ions (C2, C3, C5, C6) showed no activity while the Pt(IV) complex (C7) was as active as the original ligand against all types. Among the selected metal complexes of LIIH, the Pd(II) complex (C10) was highly potent against all bacterial cultures. These results indicate that the degree of growth inhibition is highly dependent on the structure of ligands, metal complexes, and type of metal ion [51, 52]. Although the inhibition zones of LIH, C7 and C10  were larger than that caused by Ceftriaxone, other categories, like toxicity of these compounds, still have to be studied in detail.Table 5
Antibacterial activities of the Schiff and Mannich bases and  some selected metal complexes showing inhibition zones in diameters (mm).
EntryCompoundProteus mirabilisEscherichia coliStaphylococcus aureus1SBH19++30+++29+++2LIH32++++48+++++43+++++3Co(II) (C2)——————4Pd(II) (C5)——8—9—5Ir(III) (C6)——10—9—6Pt(IV) (C7)38+++++39+++++44+++++7LIIH9—9—12—8Co(II) (C8)9—8—15+9Pd(II) (C10)38+++++39+++++44+++++10Cd(II) (C12)9—8—15+11ceftriaxone28+++30+++36++++


## 7.2. Cytotoxic Effect

Preliminary cytotoxicity tests of the Schiff base (SBH) and its Mannich base ligands (LIH and LIIH) with some selected metal complexes were performed in triplicate against cancer cell line of human epidermoid larynx carcinoma (Hep-2) using concentrations of 62.5, 125, 250, and 500 μg/mL in DMSO with exposure time of 48 h using ELISA spectrophotometer. The three organic compounds showed high toxic activities at 125, 250, 250 μg/mL, respectively, causing cell death as was confirmed by the drop in optical absorbance of NR in the treated cells compared with the controls which refers to complete disruption of cell functions [53]. The cytotoxic effect of metal complexes of LIH was found to increase in the order of Pt(IV) < Pd(II) << Ir(III) as is shown in Figure 9. The Pt(IV) complex (C7) was much less active than the parent ligand, and its performance was found to decrease with concentration that it was totally inactive at 500 μg/mL.Cytotoxic effect of LIH, LIIH, and some selected metal complexes on growth of cancer cell line Hep-2 at different concentrations with exposure time 48 h.
(a)(b)The Pd(II) complex (C5) followed the same trend of concentration as the Pt(IV) complex but it was toxic enough to cause cell death. The Ir(III) complex (C6) was exceptionally active, and its cytotoxic activity was found to increase with concentration. Figure 10 illustrates the difference in dye distribution in the tissue culture sections of Hep-2 before and after treatment with this complex in comparison with the control. Both the Pd(II) and Cd(II) complexes of LIIH (C10 and C12) were less toxic than the parent ligand, and their activity slightly increased with concentration. The Cd(II) complex (C12) caused 30–60% decrease of ligand activity. The complex was similarly inactive against growth of the three bacterial cultures although Cd++ ion is well known as an environmental carcinogen at very low concentrations in human and animals [54]. This indicates that the toxicity of Cd++ ion can be decreased on complexation with some ligands.Tissue culture sections of Hep-2 cell line before (c) and after treatment with IrLI (C6).
(a)(b)The present study describes a narrow scope of the cytotoxic activity of the studied compounds.  Extension of this study, in future work to involve other cancer cell lines and other metal complexes, using normal human cell lines as control, may reveal more important data.


## 8. Conclusions

Condensation of dithiooxamide with isatin or its N-Mannich bases occurred from one amino end of the compound which allowed for tautomerism of the resulted compound in solutions as was confirmed by1H.n.m.r spectrum of the product and from the IR spectra of some of its coordination compounds. The potent chelating behavior of the two new Mannich and Schiff bases led to the formation of bi- and polynuclear metal complexes. The preliminary study of biological activity showed some controversy in performance between bacterial growth inhibition and cytotoxic activities against Hep-2 cell line. The Ir(III) complex of LIH  which showed the highest cytotoxic effect was almost inactive against bacterial growth.



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*Source: 706262-2011-05-15.xml*