Crystal Structure and Thermal Decomposition Studies on Cobalt (II) Complex of 4-Chloro-2-((E)-(Isopropylimino)methyl)phenol
Crystal Structure and Thermal Decomposition Studies on Cobalt (II) Complex of 4-Chloro-2-((E)-(Isopropylimino)methyl)phenol
Journal of the Korean Chemical Society. 2011. Jun, 55(3): 341-345
Copyright © 2011, The Korean Chemical Society
  • Received : May 24, 2010
  • Accepted : February 21, 2011
  • Published : June 20, 2011
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Xiao-Hua, Pu

The Schiff base cobalt(II) complex, bis[4-chloro-2-(( E )-(isopropylimino) methyl) phenol]cobalt(II), has been prepared and characterized by single-crystal X-ray diffraction analyses. The phenomenological, kinetic and mechanistic aspects of the cobalt (II) complex have been studied by TG/DTG techniques. On the basis of the experimental data, the kinetic parameters such as activation energy, pre-exponential factor and entropy of activation were computed, and then the most probable mechanism function was estimated as g ( α )= α 2 . Hence the rate controlling process at all stages of decomposition is onedimensional diffusion (Parabolic model).
Transition metal complexes containing oxygen and nitrogen donor Schiff base ligands had been of research interest for many years for their industrial and biological applications. 1 - 4 Li et . al . had reported the crystal structure of bis[4-chloro-2-(cyclohexylim-inomethyl)-phenolato]-cobalt(II) and bis[4-chloro-2-(cyclohexyliminomethyl)-phenolato]zinc(II), 5 - 6 which are of great interests in coordination chemistry in relation to catalysis and enzymatic reactions, magnetism and molecular architectures. The symmetrical bis(aza crown ether)s cobalt(II) complexes had been prepared and had proven to be a model to mimic hydrolase in PNPP hydrolysis. 7 A wide variety of cobalt(II) complexes had been studied as model compounds for natural oxygen carriers and for their use in O 2 storage. 8 Even though many Schiff bases using 5-Chlorosalicy-laldehyde and amines had been studied, 9 - 12 as ligands, no work had been done with 5-chlorosalicylaldehyde and isopropylamine as the basic nucleus of Schiff bases. In addition, the thermal behaviour of this type of complex is almost unknown, because systematic thermal analysis has not been carried out.
In this paper, we report synthesis and thermal behaviour of a new cobalt(II) complex, bis[4-chloro-2-((E)-(isopropylimino) methyl)phenol]cobalt(II) ( 1 ). The structure of the complex had been established accurately from the single crystal X-ray diffraction study. The Co(II) ion in the monomeric unit seems to reside in a distorted tetrahedral environment and bonds to two oxygen atoms and two nitrogen atoms from two Schiff bases. Thermal studies supported the chemical formulation of the complex and showed that the complex decomposes in four steps. The kinetic parameters such as activation energy, preexponential factor and entropy of activation of the complex were calculated. The mechanism for the thermal decomposition process was also proposed.
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The structure of the title complex.
- Physical measurements
Thermogravimetric analyses were carried out on a Pyris Diamond TG/DTA SII thermal analyzer, Perkin Elmer. Instrument calibration was performed with standard indium samples of known melting temperature. For the kinetics measurements, about 3 mg sample was weighted in to an open platinum crucible. The selected heating rate was 5 K.min -1 , and nitrogen gas of high purity (> 99.999%) with a flow rate of 50 mL min -1 was used as carrier gas. The kinetic evaluation of the thermal decomposition of the complex was done using origin 8.0.
- Synthesis of the complex
To the vigorously stirred solution of 5-Chlorosalicylaldehyde (0.1 mmol, 15.7 mg) in EtOH (1 cm 3 ), was added dropwise a colourless solution of isopropylamine (0.1 mmol, 5.9 mg) in solution of EtOH (1 cm 3 ) with stirring at room temperature for 1 h. To the resulting orange solution was added Co(NO 3 ) 2 ·6H 2 O 0.1 mmol, 35.3 mg). The mixture was stirred for 1 h. Dark red block-shaped crystals of the title complex grew after two weeks. The product was filtered, washed with EtOH, and dried over anhydrous CaCl 2 in vacuo overnight. Yield: 90%. Anal. Calcd. (%) for (C 20 H 22 C O N 2 O 2 Cl 2 ): C, 54.09; H, 5.19; N, 6.01. Found (%): C, 54.13; H, 5.21; N, 6.05.
- X-ray single crystal structure determination
A dark red block crystal of the title complex having approximate dimensions of 0.26 mm × 0.22 mm × 0.11 mm was mounted on a glass fiber in a random orientation. The data were collected on a Bruker SMART 1000 CCD diffractometer at 298(2) K. The unit cell parameters and data collections were performed using Bruker SMART program 13 with graphite-monochromatic MoKα radiation (λ=0.71073Å). Semiempirical absorption correction was applied by using the SADABS program. 14 The structure was solved by direct methods and refined by full-matrix least-squares techniques on F 2 using the SHELXL-97 program package. 15 All the non-hydrogen atoms were refined anisotropically, and hydrogen atoms were located at their idealized positions. The crystal data and structure refinement parameters for the complex are summarized in 1 . Selected bond lengths and angles are given in 2 .
Crystal data and structure refinement parameters
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Note: R1=Σ||Fo| − |Fc||/|Fo|, wR2= Σ[w(FO2)2w(FO2)]1/2, w1=[σ2(FO2)2+ (0.0612(FO2 + 2FC2)/3)2 + 0.0000(FO2 + 2)/3)]-1
Selected bond lengths and bond angles
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Symmetry codes: (A) -x+1,y,-z+3/2
- Description of the crystal structure
The structure of the complex including atom-numbering scheme, is shown in . 1 . The X-ray diffraction analysis of the complex shows, that the central cobalt(II) atom is four coordinate and bonds to two nitrogen atoms and two oxygen atoms from two 4-chloro-2-(( E )-(isopropylimino) methyl)phenol Schiff bases in the usual trans arrangement. Each Schiff base acts as a bidentate ligand. The geometry around cobalt(II) is in a distorted tetrahedral environment, where the dihedral angle between the two coordination planes defined by O1Co1N1 and O1ACo1N1A is 86.60 o , nearly perpendicular, which could be interpreted in terms of the isopropyl substituent having a bigger steric effect than the diphenylmethyl substituent on the geometry of these kinds of complexes. 16 The phenyl ring plane (C2/C3/C4/C5/C6/C7) and the chelate ring (O1/Co1/N1/C1/C2/C3) are nearly coplanar with a dihedral angle of 3.4(2) o . This is true of the corresponding planes which were generated by symmetry. Bond angles also show that the coordination geometry about the cobalt atom is a distorted tetrahedral structure, with O1Co1N1, N1Co1N1A and O1Co1O1A angles of 96.39(11), 117.75(17) and 119.79(15), respectively. The Co1O1 and Co1N1 distances are 1.913(3) and 1.992(3) Å, respectively, which are approached to the values found in other four coordinate cobalt complexes with similar ligands. 5 , 8 Discrete monomeric molecules in both structures are held together by weak intermolecular interactions of cobalt atom with H8 and weak hydrogen bonds C9-H9---C2, which connect the independent molecules to form a onedimentional chain ( . 2 ).
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Molecular structure of the title complex. Displacement ellipsoids are drawn at the 30% probability level.
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The packing structure of the complex along the b-axis, showing the formation of 1D-chains by weak intermolecular Co….H interactions and weak hydrogen bonds C9-H9---C2.
- Phenomenological aspect
The thermal behavior of the complex was characterized using TG/DTG methods. The TG/DTG measurements of the complex were carried out within a temperature range from room temperature up to 800 ℃. Typical thermogram of the complex is shown in . 3 . The complex undergoes a four-stage decomposition pattern in the range 107-582 ℃. The first decomposition stage starts at 107 and ends at 167 ℃ with the DTG peak at 133 ℃. The corresponding mass loss (9.5%) is attributed to the loss of the adsorbed water molecules. 17 The second stage of decomposition starts at 194 and comes to an end at 345 ℃ with the DTG peak at 330 ℃. The corresponding mass loss is 11.57% (calcd. 12.17%), which is associated with the decomposition of one (CH 3 ) 2 C-N group of the ligand. Partial decomposition starts with the third step, which follows immediately after the second step in the 345-414 ℃ range with DTG peak at 387 ℃. This step includes separation of the other (CH 3 ) 2 C-N from the ligand with a mass loss 11.21% (calcd. 12.17%). The remaining part of the ligand is lost in the 414-590 ℃ range where the final decomposition takes place at 520 with metal carbonate as the residue. 18
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TG and DTG curves of the complex.
- Kinetic aspect
According to non-isothermal kinetic theory, thermal decomposition process can be described by Coats-Redfern equation. 19
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The kinetic parameters such as the activation energy ( Ea ) and the pre-exponential factor ( A ) are also calculated by this equation, where T –absolute temperature, A –preexponential factor, R –gas constant, φ –heating rate and Ea –activation energy.
The assignment of the specific mechanism of thermal decomposition is based on the assumption that the form of g (α) depends on the reaction mechanism. On plotting log[ g (α)/ T 2 ] vs. 10 3 / T calculated from TG trace for thirtyseven types 20 of mechanism functions, the most probable mechanism corresponding to the linear plot can be estimated. 21
The correlation coefficient r (as shown in 3 ) are obtained by plotting log[ g (α)/ T 2 ] vs. 10 3 / T . The parameters show that the correlation coefficient of No. 1 is better than others, and therefore g ( α )= α 2 would be the most probable mechanism function in all stages of decomposition. The mechanism of decomposition is one-dimensional diffusion. This represents the “Parabolic model”.
The entropy of activation (Δ S ) is also calculated for each stage of thermal decomposition in the complex using the following relationship,
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where A –pre-exponential factor, k –Boltzmann constant, Ts –peak temperature, DS –entropy of activation and R –gas constant.
Correlation coefficients calculated using thirty-seven forms ofg(α) for the complex
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Correlation coefficients calculated using thirty-seven forms of g(α) for the complex
Kinetic parameters for thermal decomposition of the complex
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Kinetic parameters for thermal decomposition of the complex
The activation energy ( Ea ), pre-exponential factor ( A ) and entropy of activation (Δ S ) for stages II-IV of decomposition are listed in 4 . The negative values of entropy of activation indicate that the activated complex has a more ordered structure than the reactants. 22
A new complex of Co(II) with Schiff base was synthesized and the structure was determined by X-ray crystallography study.
The TG data reveal that the complex undergoes a fourstage solid state thermal decomposition pattern. The kinetic model function was g ( α )= α 2 . The kinetic parameters such as activation energy, pre-exponential factor and entropy of activation of the complex were calculated. The mechanism for the different decomposition stages is found to be one-dimensional diffusion (Parabolic model).
Supplementary material: CCDC 773456 contains the supplementary crystallographic data for this paper. These data can be obtained free of charge at [or from the Cambridge Crystallographic Data Center (CCDC), 12 Union Road, Cambridge CB2 1EZ, UK; fax:+44(0)1223-336033; email: ].
We are grateful to the support of the research grant of Phytochemistry Key Laboratory of Shaanxi Province of the People's Republic of China. (No. 09JS068).
Chen D. , Martell A. E. , Sun Y. Z. 1989 Inorganic Chemistry 13 2647 -    DOI : 10.1021/ic00312a029
Elmali A. , Zeyrek C. T. , Elerman Y. , Durlu T. N. 2000 Journal of Chemical Crystallography 3 167 -    DOI : 10.1023/A:1009526913565
Chakraborty J. , Samanta B. , Pilet G. , Mitra S. 2006 Struct. Chem. 17 585 -    DOI : 10.1007/s11224-006-9076-3
Yilmaz I. , Ilhan S. , Temel H. , Kilic A. 2009 J. Incl. Phenom. Macrocycl. Chem. 63 163 -    DOI : 10.1007/s10847-008-9502-9
Li Z. X. , Zhang X. L 2005 Acta. Cryst. E61 o2806 -
Li Z. X. , Zhang X. L. 2005 Acta. Cryst. E61 m1755 -
Zhang C. G. , Tian G. H. , Liu B. 2000 Transition Metal Chemistry 25 377 -    DOI : 10.1023/A:1007097429960
Deligönü N. , Tümer M. , Serin S. 2006 Transition Metal Chemistry 31 920 -    DOI : 10.1007/s11243-006-0087-0
Li Z. X. , Zhang X. L. , Wang X. L. 2006 Acta. Cryst. E62 o4513 -
Zhang X. L. , Li Z. X. 2007 Acta. Cryst. E63 o319 -
Kabak M. , Elmali A. , Kavlakoğlu E. , Elerman Y. , Durlu T. N. 1999 Acta. Crystallogr. C55 1650 -
Patel N. H. , Parekh H. M. , Patel M. N. 2005 Transition Metal Chemistry 30 13 -    DOI : 10.1007/s11243-004-3226-5
Bruker (2000) SMART (Version 5.0) and SAINT (Version 6.02). Bruker AXS Inc. Madison, Wisconsin, USA.
Sheldrick G. M. SHELXTL. 1995 Structure Determination Soft ware Suite. Siemens Industrial Automation, Analytical Instrumentation USA
Sheldrick G. M. SADABS. 1997 Siemens area detector absorption (and other) correction. University of Göttingen Germany
Fernández-G J. M. , Ruíz-Ramírez O. L. , Toscano R. A. , Macías-Ruvalcaba N. , Aguilar-Martínez M. 2000 Transition Metal Chemistry 25 511 -    DOI : 10.1023/A:1007028814788
Deligönül N. , Tümer M. 2006 Transition Metal Chemistry 31 920 -    DOI : 10.1007/s11243-006-0087-0
Mohamed G. G. , Abd El-Wahab Z. H. 2003 Journal of Thermal Analysis and Calorimetry 73 347 -    DOI : 10.1023/A:1025126801265
Coats A.W. , Redfern J. P. 1964 Nature 201 68 -    DOI : 10.1038/201068a0
Hu R. Z. , Gao S. L. , Zhao F. Q. , Shi Q. Z. , Zhang T. L. , Zhang J. J. 2008 Thermal analysis kinetics (section two) Science press Perkin China
Satava V. 1971 Thermochim. Acta. 2 423 -    DOI : 10.1016/0040-6031(71)85018-9
Mathew S. , Nair C. G. R. , Ninan K. N. 1989 Thermochim. Acta. 155 247 -    DOI : 10.1016/0040-6031(89)87150-3