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Synthesis and Spectral Characterization of Lanthanide Complexes Derived from 2-[(4-Bromo-2,6-Dichloro-Phenylimino)-Methyl]-4,6-Diiodo-Phenol

V. R. Rajewar 1, M. K. Dharmale2 , S. R. Pingalkar1

1Department of Chemistry N.E.S.Science College ,Nanded (M.S), India.

2Department of Chemistry Yeshwant Mahavidyalaya ,Nanded (M.S), India.

DOI : http://dx.doi.org/10.13005/ojc/300471

Article Publishing History
Article Received on :
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Article Published : 17 Dec 2014
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ABSTRACT:

The solid complexes of La(III), Pr (III), Tb(III) ,Sm(III) and Nd(III) were prepared from bidentate Schiff base, 2-[(4-bromo-2,6-dichloro-phenylimino)-methyl]-4,6-diiodo-phenol. The Schiff base ligand was synthesized from 3,5 diiodosalicylaldehyde and 4-bromo-2,6-dichlorobenzenamine . These metal complexes were characterized by molar conductivity, magnetic susceptibility, thermal analysis, X-ray diffraction, FTIR, 1H-NMR and UV-Vis. The analytical data of these metal complexes showed metal:ligand ratio of 1:2 La(III), Pr (III), Tb(III) ,Sm(III) and 1:1 for Nd(III) complexes. The physico-chemical study supports the presence of octahedral geometry around La(III), Pr (III), Tb(III) ,Sm(III) and Nd(III) ions. The IR spectral data reveal that the ligand behaves as bidentate with ON donor atom sequence towards central metal ion. The molar conductance values of metal complexes suggest their electrolyte nature except Nd(III) complex.
The X-ray diffraction data suggest monoclinic crystal system for Pr (III), Nd (III) complexes. Thermal behavior (TG/DTA) shows breakdown of complexes.

KEYWORDS:

Bidentate Schiff base; Metal complexes; Thermal analysis; XRD

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Rajewar V. R, Dharmale M. K, Pingalkar S. R. Synthesis and Spectral Characterization of Lanthanide Complexes Derived from 2-[(4-Bromo-2,6-Dichloro-Phenylimino)-Methyl]-4,6-Diiodo-Phenol. Orient J Chem 2014;30(4).


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Rajewar V. R, Dharmale M. K, Pingalkar S. R. Synthesis and Spectral Characterization of Lanthanide Complexes Derived from 2-[(4-Bromo-2,6-Dichloro-Phenylimino)-Methyl]-4,6-Diiodo-Phenol. Available from: http://www.orientjchem.org/?p=5976


Introduction

Schiff bases derived from aromatic amines and aldehydes have a wide variety and an important class of ligands in coordination chemistry and find extensive applications in different fields, e.g., biological, inorganic and analytical chemistry 1.2. Many biologically important Schiff bases have been reported in the literature possessing, antimicrobial, antibacterial, antifungal, anti-inflammatory, antitumor and anti HIV activities 3.4. Schiff bases play important roles in coordination chemistry as they easily form stable complexes with most transition metal ions 5.

The interaction of these donors ligands and metal ions give complexes of different geometries and these complexes are potentially biologically active6. Several research papers reported the synthesis and characterization of transition metal complexes of Schiff bases derived from salicylaldehyde7,8.

Metal complexes with Schiff base ligands containing salicylaldehyde and its derivatives; have been extensively studied. Metal complexes with such ligands are quite common and also reflect their facile synthesis, accessibility of diverse structural modifications and wide applications in different fields, such as catalysis, biological systems and material chemistry9, 10.

Transition metal complexes with Schiff base as ligand have been amongst the widely studied co-ordination compounds in the past few years, since they are found to be widely applicable in many fields such as biochemical, analytical and antimicrobial fields11-15. It is well known from the literature that much work have been done on the synthesis and characterization of this compounds16-18 with Schiff base ligand formed from salicylaldehyde or substituted salicylaldehyde and various aromatic amines19-23.

Salicylic aldehyde is an important intermediate in the manufacture of herbicides  and pesticides.28

Also, salicylaldehyde and its derivatives are used for various reactions for the production of polymers and fibers.

Salicylaldehyde is called 2-hydroxybenzaldehyde and ortho-hydroxy benzaldehyde and is an organic compound with the formula C7H6O2. Part of the class hydroxy aromatic aldehydes, aromatic nucleus contains two functional groups: a hydroxyl and aldehyde one. This colorless liquid has a bitter almond odor at higher concentrations The natural oils found in Spiraea [Filipendula (Spiraea) ulmaria (Rosaceae)].

Sweet-smelling flowers containing salicylaldehyde and methyl salicylate, glycosides form. Was also identified as a component of the characteristic flavor of buckwheat.24 Salicilaldehyde is used as an important intermediate in the chemical industry, in medicine. It is used in perfume, fragrances, dyes, pharmaceuticals, etc.25 Salicylaldehyde and its derivatives can be used as preservatives in cosmetic products, 26 fragrances, essential oils in various biological applications.27  Also get in formulation of perfumes and fragrances.

Experimental

All chemicals and solvents are used AR grade. All the metals were used as their chloride salts. UV spectra recorded on UV-vis spectrophotometer 119. Conductance or metal complex was determined in DMSO on conductivity meter quiptronics model NO-EQ665. Melting points were recorded on in recorded by open capillary method and are uncorreded. H1-NMR spectra or a Schiff base and its metal complex recorded on Brukcer 300 MHz spectrometer in DMSO. Elemental analysis was carried out on Eager 350 analyser. Magnetic measurement were done on solid complexes using Guoy method. Powder XRD pattern of complexes are recorded Philips Analytical XRD B.V. at CFC Shivaji University Kolhapur.

Synthesis of Ligand

Synthesis of 2-[(4-Bromo-2,6-Dichloro-Phenylimino)-Methyl]-4,6-Diiodo-Phenol (BDPDP) Schiff Base

Schiff base ligand were synthesized by refluxing of 3,5 diiodosalicylaldehyde (0.01M)  and 4-bromo-2,6-dichlorobenzenamine (0.01 M) in 50m1 ethanol on water bath for 4-5 hours in presence of 2-3 drops of glacial acetic acid. The reaction mixture was kept for overnight, where yellow color precipitate was obtained. It was filtered by whatmann paper, washed with distilled water then alcohol, dried in vacuum dessicator. Pure Schiff base was recrystallized from ethanol. The purity of ligand was checked by TLC.

 

Scheme 1 Scheme 1

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Synthesis of Metal Complexes

The ethanolic solution of Metal chloride (0.01M) was added to hot ethanolic solution of BDPDP (0.02 M) La(III), Pr (III), Tb(III) ,Sm(III) and (0.01 M) in  Nd(III) complexes drop wise with constant stirring. PH of the reaction mixture was adjusted to 7 -7.2 with alcoholic ammonia solution. Resulting reaction mixture refluxed for 5 to 6 hours on water bath.

Colored complexes was allowed to digest and collected by filtration. Then washed with sufficient quantity of distilled water and little hot ethanol to apparent dryness and dried in vacuum desiccators.

Results and Discussion

Physical and Analytical Parameters

Empirical formulae of the complexes were deduced on the basis of elemental analysis, metal ligand ratio and thermal analysis (table No. 1.1 and 1.2). Complexes possess different colors, metal complexes of ligand BDPDP are insoluble in common organic solvents, dissolve freely in DMSO/DMF High melting points of complexes suggest that complexes are stable at normal temperatures29. Molar conductivity (lm 71 to 82 W-1cm2mol-l) reveals electrolytic nature of the complexes30 except Neodymium metal ion complex (lm 14W-1 cm2mol-l) reveals   nonelectrolytic nature of the complex.(table 1.1).

Table 1.1: Physical and analytical data of BDPDP metal complexes.

 

Compound

F.W.

Yield

M.L ratio

M.P.

decom.

Temp °C

Color

 

Molar

Conductance W-1  cm2 mol-1

%of Cl cal. (obs)

Magnetic Moment

BDPDP(L)

596.81

67 %

—-

1900C

Yellow

—-

—-

—-

[La(L)22H2O]Cl

1404.01

58 %

1:2

>270 0C

Muddy Yellow

66

12.63 (12.59)

Dimagnetc

[Pr(L)22H2O]Cl

1408.03

62 %

1:2

>270 0C

Brown

71

12.59   (12.57)

Paramagnetic

[Nd(L)12H2O2Cl]

847.99

58 %

1:1

>270 0C

Grey

14

16.72 (16.74)

Paramagnetic

[Tb(L)22H2O]Cl

1426.05

51 %

1:2

>270 0C

Dark Yellow

78

12.43 (12.41)

Paramagnetic

[Sm(L)22H2O]Cl

1412.33

61 %

1:2

>270 0C

Faint Yellow

64

12.52 (12.48)

Paramagnetic

 

Table 1.2: Percent C, H, N,O and metal ion in BDPDP metal complexes.

Compound

Empirical Formula

%C obs (calcd.) %H obs (calcd.) %N obs (calcd.) %O obs (calcd.) % I obs (calcd.) % Br obs (calcd.) %M obs (calcd.)
 BDPDP(L) C13H6BrCl2I2NO

26.16 (26.12)

1.01 (0.92)

2.35 (2.24)

2.68 (2.46)

42.53 (42.42)

13.39 (13.12)

—-

[La(L)22H2O]Cl C26H16Br2Cl5I4LaN2O4

22.24 (22.14)

1.15 (1.11)

2.00 (1.98)

4.56 (4.31)

36.15 (36.23)

11.38 (11.23)

9.89 (9.78)

[Pr(L)22H2O]Cl C26H18Br2Cl5I4N2O4Pr

22.18 (22.09)

1.29 (1.14)

4.55 (4.34)

4.55 (4.43)

36.05 (35.95)

11.35 (11.27)

10.01 (9.67)

[Nd(L)12H2O2Cl] C13H10BrCl4I2NNdO3

18.41 (18.31)

1.19 (1.04)

1.65 (1.45)

5.66 (5.45)

29.93 (29.84)

9.42  (9.31)

17.01 (16.47)

[Tb(L)22H2O]Cl C26H18Br2Cl5I4N2O4Tb

21,90 (21.87)

1.27 (1.16)

1.96 (1.89)

4.49 (4.38)

35.60 (35.49)

11.21 (11.14)

11.14 (11.03)

[Sm(L)22H2O]Cl C26H16Br2Cl5I4N2O4Sm

22.06 (21.89)

1.14 (1.08)

1.98 (1.78)

4.52 (4.43)

35.86 (35.73)

11.29 (11.18)

10.62 (10.54)

 

Electronic Spectra

Plots of  UV-Visible spectra of ligand BDPDP and its metal complexes were recorded on UV-Visible spectrophotometer 119-Pc based instrument are presented in figure 6.1, 6.2, 6.3 , 6.4,6.5 and 6.6. Ligand (BDPDP) shows strong absorption band at 34160 cm-1 assigned for  π – π*  transition. Absorption bands and corresponding transition are given in the table No. 1.3.

Table 1.3: Electronic spectral data of BDPDP complexes.

 

Ligand / Complex

Absorbance nm

n/cm-1

Transition

BDPDP(L)

293

34160

π – π*

[La(L)22H2O]Cl3

261

38314

π – π*

431

23201

LMCT

  • [Pr(L)22H2O]Cl

261

38314

π – π*

431

23201

LMCT

  • [Nd(L)12H2O2Cl]

259

38610

π – π*

431

23201

LMCT

  • [Tb(L)22H2O]Cl

261

38314

π- π*

429

23310

LMCT

  • [Sm(L)22H2O]Cl

261

38314

π- π*

429

23310

LMCT

 

The UV electronic spectra of La(III), Pr (III), Nd(III), Tb(III) and Sm(III)complexes  have indicates absorption bands at 23201 cm-1, 23201 cm-1, 23201 cm-1,23310 cm-1 and 23310 cm-1 assigned as charge transfer31,32.

Infrared Spectra

Determination of coordinating atoms in the complex is made on the basis of comparison of IR spectra of the ligand and their metal complexes. Significant changes in wave numbers of the coordinating atoms involved in coordination are summarized in the table No. 1.4.

IR Spectral Study of BDPDP Ligand 

Ligand BDPDP contains phenolic –OH and azomethine  group. In spectra of ligand exhibits strong n (O-H) stretching at 3447 cm-1, corresponding to n (OH) of phenol. The band at 1204cm-1 is due to presence of n (C-O) group. It also indicate n (C=N) stretching frequency at 1616cm-1. On complexation significant changes in wave numbers are observed.

IR Spectral Study of La(III) Complex

The IR spectra of  Metal complexes   is compared with IR spectra of ligand (BDPDP), there are certain shifts in the bands. In complex deprotonation of —OH in phenolic group and indicating involvement of phenolic group in coordination 33. The band stretching vibration in ligand due to phenolic n(OH) group observed at 3447cm-1, Which is disappear in complex.

Besides, ligand exhibits stretching of  n (C=N) stretching at 1616cm-1 which on complexation  shifted to lower wave number at 1596-1631cm-1suggesting that azomethine  nitrogen are involved in coordination34′ 35 .A new broad  band at 3134-3477cm-1 suggested  the presence of coordinated water molecule36.

The appearance of new bands in the spectra of metal ion complex at 432-441cm-1 and 505-520 cm-1 due to new bonding i.e. n (M-N) and n (M- O)37,38.

Thus the ligand BDPDP exhibits uninegative bidentate behaviour and coordinates to the metal ion through azomethine  nitrogen and phenoxide oxygen for La(III), Pr (III), Tb(III) and Sm(III)complexes, Nd(III) complex behave neutral in nature.

Table No 1.4  Infrared spectral data of the ligand (DPMDI) and their La(III), Pr (III), Nd(III), Tb(III) and Sm(III) metal complexes

 

Compound

n(CH=N)

n(C-O)

n(M-O)

n(M-N)

n(H2O) Rocking

n(H2O)

n(OH)

BDPDP(L)

1616

1204

—-

—-

—-

—-

3447

[La(L)22H2O]Cl

1596

1212

520

432

853

3134

—-

[Pr(L)22H2O]Cl

1627

1209

505

432

860

3477

—-

[Nd(L)12H2O2Cl]

1629

1211

507

435

869

3448

—-

[Tb(L)22H2O]Cl

1627

1211

507

441

889

3437

—-

[Sm(L)22H2O]Cl

1631

1211

509

435

867

3473

—-

 

1HNMR Spectra

1H NMR spectral studies of ligand BDPDP indicated signals at d 6.9- 7.2 ppm corresponding to aromatic protons (m, 4H, Ar-H) and at d 7.9 ppm due to azomethine group  (CH=N). A strong signal at d 13.3 ppm assignable (S, 1H) due to phenolic OH group (fig. 1.1).

In the metal complex signal corresponding to phenolic OH group at d 13.3 ppm has disappeared39-41 (fig.1.2) may be attributed to deprotonation of —OH group on involvement of via -OH in bonding. A new peak due to presence of coordinated water at d 2.5 ppm is observed in  metal complex42 .The shift in azomethine group from d 7.9 ppm to d 9.6 ppm indicate coordination through water molucule  azomethine group.

Thus, BDPDP.molecule seems to be coordinated to the metal through phenoxide  oxygen  and azomethine group  in  Pr (III) metal  complex.

 

Figure 6.13:1H NMR ligand BDPDP  Figure6.13: 1H NMR ligand BDPDP   

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Figure 1.2:1H NMR Metal complex Figure1.2: 1H NMR Metal complex 

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Thermal Study

Nd(III), Pr(III) and Tb(III) complexes were studied by therrnogravimetric analysis from ambident temperature to 1000°C in nitrogen atomosphere.   The range of temperature, experimental and calculated mass losses of the decomposition reaction are given in the table No. 1.5. TGA/DSC scans are depicted in figures 1.3, 1.4 and 1.5.

Thermal Study of [Tb(L)22H2O]Cl

The thermogram of Tb(III) complex shows weight loss 2.44% corresponding to two coordinated  water molecule in the range from room temperature to 140°C. Decomposition reaction corresponds to an experimental mass  2.42 % occurs in the temperature range 140°C- 280°C attributed loss of  one lattice chlorine 43. part of the complex.

In the temperature range 280°C-310°C Four iodine part is lost and this loss corresponds to 38.04%. As the temperature increases to 310-600°C there is of 18.16 % indicating loss of four chloride,two bromine , part of metal complex. From 600-8000C loss of organic moiety which is 28.12 %.Finally 800°C-1000°C residue is obtained corresponding to Tb2O3 as stable residue 44 12.44%.

Thermal Study of [Pr(L)22H2O]Cl

The TGA of Pr(III) complex indicates loss in weight in the range from room temperature to 160°C corresponding to 2.32 % indicates the loss of coordinated water-molecule.

Decomposition beyond this temperature in the range 160°C -390°C corresponds to mass loss of  61.32 % in the TG curve assigned to expulsion of one lattice chloride molecules four iodine, four chloride ,  two bromine   part of the complex. The decomposition occurs in the temperature 390°C -800°C indicates the loss of Organic Moiety  27.68 %. Further at 800°C-1000°C losses of 11.87 % were occurs indicating  presence of thermally stable residual metal oxide45.

Thermal Study of [Nd(L)12H2O2Cl]

TGA of Nd (III) complex shows weight loss corresponding to mass loss 4.25 %. This loss corresponds to loss of coordinated water molecule in the range from room temperature to 160°C46. Further decomposition at 160°C-430°Closs of 36.71 % was occurs indicating loss of Two iodine, One bromine  of the complex. From 430-8000C loss of four chlorine , Organic moiety which is  33.64 %.The end product of decomposition is formation of Nd2O3 weight corresponds to 19.58 percent which is equal to theoretical value 20.09.

Table-1.5 Thermal Analysis data for metal complexes

Complex Decomposition Temp°C Lost fragment

Weight loss %

Experimental

Theoretical

[Tb(L)22H2O]Cl 140oC two coordinate water molecule

2.44

2.56

140-280 oC one lattice chlorine

2.42

2.53

280-310 oC Four iodine

38.04

36.22

310-600 oC Four chlorine two bromine

18.16

21.53

600-800 oC Organic moiety

28.12

27.23

800-1000 oC Metal oxide

12.44

13.04

[Pr(L)22H2O]Cl 160oC two coordinated  Water molecules

2.32

2.60

160-390 oC one lattice chloride molecules four iodine, four chloride ,  two bromine

61.32

61.02

390-800 oC Organic Moiety

27.68

26.64

800-1000 oC Metal oxide

11.87

11.91

[Nd(L)12H2O2Cl] 160 oC coordinated two water molecules

4.25

4.30

160-430 oC Two iodine, One bromine

36.71

39.89

430-800 oC four chlorine , Organic moiety

33.64

32.60

800-1000 oC Metal oxide

19.58

20.09

 

Figure 1.3: TG/DSC [Tb(L)22H2O]Cl Figure1.3: TG/DSC [Tb(L)22H2O]Cl  

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Figure 1.4: TG/DSC [Nd(L)12H2O2Cl] Figure1.4: TG/DSC [Nd(L)12H2O2Cl]  

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 Figure 1.5: TG/DSC  [Pr(L)22H2O]Cl

Figure1.5: TG/DSC  [Pr(L)22H2O]Cl  

 

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Powder X-Ray Studies

X-ray diffractograms of the metal complexes were recorded in the 2q range from 10-90° at a wave length of  1.5405 A°and using Cu Ka radiation source. Results of miller indices, lattice parameters and unit cell volume are computed from programmer. Data has been summarized in the following tables.

[Nd(L)12H2O2Cl]

Crystal system:  Monoclinic  Lattice Type: P

Lattice Parameter:  a= 9.53034  b= 8.00951  c=  7.79302   A0

Lattice Parameter: Alpha= 90.000  Beta= 121.572   Gama=90.000

h    k     l

2θ (cal )

2θ (Obs)

d(cal)

d (obs)

-1     0   1

6.00366

6.01408

7.36480

7.34506

-1     1   0

7.76464

7.75704

5.70152

5.70286

-2     0   0

10.94017

10.92606

4.05882

4.06188

-2     1   2

13.31070

13.30282

3.34576

3.34628

-2     2   1

14.58616

14.57042

3.05874

3.06078

-4    1   0

23.05168

23.04753

1.96725

1.96712

3     0    2

26.85357

26.85035

1.70529

1.70514

-4    2   5

32.39762

32.39613

1.43768

1.43751

-1    5   3

34.86598

34.85211

1.34748

1.34775

-2    6    1

36.83277

36.83274

1.28494

1.28477

-2    1    6

38.73699

38.73415

1.23101

1.23093

-4    3    6

41.28170

41.26937

1.16754

1.16769

-4    6    3

42.69762

42.69542

1.13592

1.13584

 

 Figure 1 Figure 1
Click here to View figure

 

The cell data and crystal parameters of [Nd(L)12H2O2Cl]  complex is given in the tables indicates that complex have monoclinic crystal system47, with lattice type-P.

[Pr(L)22H2O]Cl

Crystal system:  Monoclinic  Lattice Type: P

Lattice Parameter:  a= 19.06907  b= 4.64343  c=  7.04556 A0

Lattice Parameter: Alpha= 90.000  Beta= 108.476   Gama=90.000

h     k      l

2θ (cal )

2θ (Obs)

d(cal)

d (obs)

-2     0    1

6.87288

6.88556

1.27114

6.43274

1     0     1

7.75612

7.75704

5.70775

5.71298

2     0     1

9.41625

9.42077

4.70827

4.71002

-1     1    1

11.46505

11.48063

3.87533

3.87282

1     1     1

12.34822

12.35211

3.60201

3.60321

1     0     2

14.32149

14.33275

3.11405

3.11337

-7     0    2

18.28842

18.29401

2.45474

2.45506

0     2     2

23.82950

23.83979

1.90660

1.90644

8     1     2

29.77117

29.78169

1.55134

1.55123

0     3     3

37.30260

37.30810

1.27107

1.27114

 

Figure 2 Figure 2

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Cell data and crystal lattice parameters of  [Pr(L)22H2O]Cl  complex attributed to monoclinic crystal system48, with lattice type-P.

Proposed Structures of the Chelates

Based on above result probable structure have been proposed

 

Figure 3 Figure 3

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