Structures and Magnetic Properties of Monomeric Copper(II) Bromide Complexes with a Pyridine-Containing Tridentate Schiff Base
Structures and Magnetic Properties of Monomeric Copper(II) Bromide Complexes with a Pyridine-Containing Tridentate Schiff Base
Bulletin of the Korean Chemical Society. 2013. Dec, 34(12): 3615-3620
Copyright © 2013, Korea Chemical Society
  • Received : July 16, 2013
  • Accepted : September 10, 2013
  • Published : December 20, 2013
Export by style
Cited by
About the Authors
Sung Kwon, Kang
Department of Chemistry, Chungnam National University, Daejeon 305-764, Korea
Soon Jung, Yong
Young-Kwang, Song
Young-Inn, Kim

Two novel copper(II) bromide complexes with pyridine containing Schiff base ligands, Cu(pmed)Br 2 and Cu(dpmed)Br 2 where pmed = N '-((pyridin-2-yl)methylene)ethane-1,2-diamine (pmed) and dpmed = N,N diethyl- N '-((pyridin-2-yl)methylene)ethane-1,2-diamine (dpmed) were synthesized and characterized using Xray single crystal structure analysis, optical and magnetic susceptibility measurements. Crystal structural analysis of Cu(pmed)Br 2 showed that the copper(II) ion has a distorted square-pyramidal geometry with the trigonality index of τ = 0.35 and two intermolecular hydrogen bonds, which result in the formation of two dimensional networks in the ab plane. On the other hand, Cu(dpmed)Br 2 displayed a near square-pyramidal geometry with the value of τ = 0.06. In both compounds, the NNN Schiff base and one Br atom occupy the basal plane, whereas the fifth apical position is occupied by the other Br atom at a greater Cu-Br apical distance. The reported complexes show g⎟⎜ > g⊥ > 2.0023 with a d x2-y2 ground state and a penta-coordinated square pyramidal geometry. Variable temperature magnetic susceptibility measurements showed that the developed copper(II) complexes follow the Curie-Weiss law, that is there are no magnetic interactions between the copper(II) ions since the Cu--Cu distance is too far for magnetic contact.
Nitrogen based Schiff base ligands and their metal complexes have been widely studied due to their versatile steric and electronic properties, 1 - 5 which can be fine-tuned by choosing appropriate amine precursors and ring substituents. In addition, they are potential models for a number of important biological systems and have possible applications as molecule-based magnetic materials. 6 - 13 The metal halide complexes of less flexible tridentate ligands tend to be monomeric and dimeric in nature, whereas the use of more flexible tridentate ligands tends to give rise to dimeric or polymeric complexes. 14 - 21 These complexes also exhibit interesting magnetic behaviours. For example, it has been found that the strengths of magnetic interactions between copper(II) metal ions are primarily a function of Cu–X…Cu contact, Cu(II) center geometry, Cu–X…X–Cu distance, Cu–X…X angle, and the electronic nature of the halide ion in copper(II) halide complexes. 22 - 23 Recently, our focus has been on the transition metal chemistry of N3 tridentate Schiff base ligands, and particularly, on mixed imino–pyridine ligands. 24 - 28 The design of such ligands incorporating different transition metals and studies of their structural and magnetic properties are in progress. Here, we describe the complexing abilities of two new Schiff-base tridentate ligands containing pyridyl, imine, and amino donor atoms, that is, N' -((Pyridin-2-yl)methylene)ethane-1,2-diamine = pmed) and, N,N -diethyl- N' -(((Pyridin-2-yl)methylene)ethane-1,2-diamine = dpmed) for Cu(II) bromide and the optical and magnetic properties of Cu(pmed)Br 2 and Cu(dpmed)Br 2 from a structural perspective.
All reagents and solvents used for syntheses and analyses were purchased from the Aldrich Chemical Company and used as received.
Preparation of Schiff Base. The Schiff base ligands, N' - ((pyridin-2-yl)methylene)ethane-1,2-diamine (pmed) and N,N -diethyl- N' -((pyridin-2-yl)methylene)ethane-1,2-diamine (dpmed) were prepared by reacting 2-pyridinecarboxaldehyde with ethylenediamine or N,N' -diethylethylenediamine, respectively. The synthetic pathway is shown in Scheme 1 .
PPT Slide
Lager Image
Synthesis of Copper(II) Complexes. Cu(pmed)Br2. A solution of CuBr 2 (1.12 g, 5 mmol) in 30 mL methanol was added dropwise with constant stirring to a methanolic solution (30 mL) of pmed ligand (0.75 g, 5 mmol), and the reaction mixture was stirred for a further 24 h at room temperature. The bluish green precipitates formed were isolated by filtration, washed with methanol and dried under vacuum. Yield: 1.34 g (72%). Anal. Calc. for Cu(C 8 H 11 N 3 )Br 2 : C, 25.79; H, 2.98; N, 11.28. Found: C, 25.61; H, 2.93; N, 11.37%. IR (KBr, cm −1 ): ν(N-H) 3259, 3230; ν(C=N) 1602; δ (Py) 764. UV–Vis (CH 3 CN; λ max ): 749, 285 nm.
Cu(dpmed)Br2. This compound was obtained in manner similar to that used to produce Cu(pmed)Br 2 , but dpmed was used instead of pmed. Dark green colour. Yield: 1.52 g (71%). Anal. Calc. for Cu(C 12 H 19 N 3 )Br 2 : C, 33.62; H, 4.47; N, 9.80. Found: C, 32.25; H, 4.96; N, 9.52%. IR (KBr, cm −1 ): ν(C=N) 1599; δ (Py) 644. UV–Vis (CH 3 CN; λ max ): 765, 289 nm.
Physical Measurements. Elemental analyses (C, H and N) were carried out at the Korean Basic Science Institute at Daejeon. IR spectra were obtained using KBr pellets and a Jasco FT-IR spectrophotometer. Electronic absorption spectra were recorded at ambient temperature on a Shimadzu UV- 3101PC spectrophotometer. The X-band EPR spectra of powder materials and frozen glass samples (toluene/methanol) at 77 K were recorded on an ESP-300S EPR spectrometer. The field modulation frequency was 100 kHz and diphenylpicrylhydrazyl (DPPH) was used as a reference. Magnetic susceptibilities were measured at different temperatures using a Magnetic Property Measurement System (MPMS7) Quantum Design and the SQUID method. Susceptibility data were corrected for the diamagnetism of constituent atoms using Pascal’s constants and for the temperature- independent paramagnetism of copper, which was estimated to be 60 × 10 −6 cgsu/Cu atom.
X-ray Single Crystal Structural Analysis. X-ray intensity data were collected on a Bruker SMART APEX-II CCD diffractometer using graphite monochromated Mo Kα radiation (λ = 0.71073 Å) at a temperature of 296 K. The structures were solved using the direct method and refined by full-matrix least-squares calculation on F2 using SHELXL- 97. All non-hydrogen atoms were refined anisotropically. Amine H atoms were located in a difference map and refined freely using refined distances of N-H = 0.80 (4) and 0.92 (4) Å. Other H atoms were positioned geometrically and refined using a riding model, with C-H = 0.93-0.97 Å with U iso = 1.2 U eq (carrier C) for aromatic- and methylene-H, and U iso = 1.5 U eq (carrier C) for methyl-H atoms.
Results and Discussion
The reaction of equimolar amounts of copper(II) bromide and tridentate Schiff-base ligands (pmed/dpmed) leads to the formation of the monomeric copper(II) complexes, Cu(pmed)Br 2 and Cu(dpmed)Br 2 without any coordinating solvent molecules as revealed by elemental analyses and Xray single crystal analyses.
Description of Structures. Single crystals of Cu(pmed)Br 2 and Cu(dpmed)Br 2 were grown from slowly evaporating solutions of acetonitrile/hexane. Crystallographic data and structure refinement parameters are summarized in Table 1 . ORTEP views including the atomic numbering scheme are shown in Figures 1(a) and 1(b) for Cu(pmed)Br 2 and Cu(dpmed)Br 2 , respectively. Selected bond distances and bond angles are summarized in Table 2 .
Crystal data and details of refinement for Cu(pmed)Br2and Cu(dpmed)Br2
PPT Slide
Lager Image
Crystal data and details of refinement for Cu(pmed)Br2 and Cu(dpmed)Br2
In both compounds, Cu atoms are coordinated by two Br atoms and the three N atoms of the tridentate Schiff base ligands. Bond angles around Cu atoms are within the ranges 79.63 (10) to 110.62 (2) o and 79.32 (10) to 105.96 (2) o for Cu(pmed)Br 2 and Cu(dpmed)Br 2 , respectively. The coordination polyhedron around Cu atom is a distorted square pyramidal geometry with a structural index, τ = 0.35 in Cu(pmed)Br 2 , whereas Cu(dpmed)Br 2 exhibits a near square pyramidal environment with τ = 0.06; [τ = (α − β)/60, where α is the largest and β is the second largest trans angle in the coordination sphere; τ = 0 for a perfect square pyramidal and τ = 1 for a trigonal bipyramidal geometry]. Apical positions in both compounds are occupied by Br2 atoms, as shown in Figure 1 .
PPT Slide
Lager Image
The molecular structures of Cu(pmed)Br2 (a) and Cu(dpmed)Br2 (b), showing the atom-numbering schemes.
Selected bond lengths (Å) and angles (0) of Cu(pmed)Br2and Cu(dpmed)Br2
PPT Slide
Lager Image
Selected bond lengths (Å) and angles ( 0 ) of Cu(pmed)Br2 and Cu(dpmed)Br2
Table 2 lists the selected bond lengths and bond angles for the reported complexes. The apical Cu1-Br2 bond distances of Cu(pmed)Br 2 and Cu(dpmed)Br 2 are 2.6221(5) and 2.6094(5) Å, respectively. Longer apical Cu1-Br2 bond distances of Cu(pmed)Br 2 and Cu(dpmed)Br 2 than those of basal Cu1–Br1 (2.3992(5) for Cu(pmed)Br 2 and 2.4142((5) Å for Cu(dpmed)Br 2 ) is a common observation in square pyramidal copper(II) complexes. The dihedral angles between Cu1/N1/N8/N11 of the chelate ring and the Br1/Cu1/ Br2 plane are 89.51 (5) and 85.85 (6) o for Cu(pmed)Br 2 and Cu(dpmed)Br 2 , respectively, which are almost perpendicular to each other.
The Cu-N1 bond distances of 2.031 and 2.065 Å for Cu(pmed)Br 2 and Cu(dpmed)Br 2 , respectively, are comparable to those observed in Cu(II) complexes with a fivecoordinate system. As shown in Table 2 , the Cu1-N8 bond distance of 1.977 Å in Cu(pmed)Br 2 (1.980 Å for Cu(dpmed)Br 2 ) is shorter than those of other two Cu-N bonds, 2.016 and 2.031 Å (2.065 and 2.099 Å for Cu(dpmed) Br 2 ), which is consistent with the better π-accepting ability of imine (C=N) than aromatic or amine nitrogen. The observed Cu1-N8 bond lengths are comparable to those observed in other copper(II) complexes containing a nitrogen containing tridentate Schiff base. 36 - 40 The C7-N8 bond distance of 1.261 Å in Cu(pmed)Br 2 (1.267 Å for Cu(dpmed) Br 2 ) is much shorter than N8-C9 bond length of 1.464 Å (1.454 Å for Cu(dpmed)Br 2 ), which demonstrates the double bond character of the imine group.
PPT Slide
Lager Image
The molecular packing diagram of Cu(pmed)Br2 shows N−HLBr hydrogen bonds (dashed lines).
A structural packing diagram of Cu(pmed)Br 2 is presented in Figure 2 . In Cu(pmed)Br 2 , the H(11A) hydrogen interacts with Br(2) of the neighbouring molecule at the x, y+1, z position and the H(11B) atom binds to the Br(2) atom of another adjacent unit at the –x+1, −y, −z+2 position. These two intermolecular hydrogen interactions result in linking the molecules into a two-dimensional network along the ab plane. In Cu(dpmed)Br 2 , two mononuclear molecules are linked by intermolecular π-π interactions at a centroid-centroid distance of 3.560 Å between the C2-C3-C4 planes of pyridine rings, as shown in Figure 3 .
Optical and Magnetic Properties. The IR spectrum of Cu(pmed)Br 2 complex shows two bands at 3259 and 3230 cm −1 , characteristic of asymmetric and symmetric vibrations of a –NH 2 group engaged in intermolecular hydrogen bonding. C=N vibration frequencies, ν(C=N), appear at 1602 and 1599 cm −1 in Cu(pmed)Br 2 and Cu(pemed)Br 2 , respectively, and are in agreement with those observed in azomethine nitrogen coordinated Schiff bases complexes.
PPT Slide
Lager Image
The molecular structures Cu(dpmed)Br2, showing the intermolecular π-π interactions with dashed lines.
UV-Vis spectra in acetonitrile exhibited broad overlapping d–d absorption bands, centered at 749 nm (ε = 175 M −1 cm −1 ) for Cu(pmed)Br 2 and at 765 nm (ε = 250 M −1 cm −1 ) for Cu(pemed)Br 2 . These features are typical for five-coordinate copper(II) complexes with square pyramidal or distorted square pyramidal geometries. Based on these square pyramidal geometries, the broad absorption peaks were resolved into three peaks by Gaussian resolution ( Figure 4 ) and tentatively assigned to d z2 →d x2-y2 1 ), d xy →d x2-y2 2 ) and d xz,yx →d x2-y2 3 ). Values of [ν 1 max =1,066 nm, ε = 300 M −1 cm −1 ), ν 2 (879, 74) and ν 3 (724, 140)] and [ν 1 (1126, 43), ν 2 (893, 99) and ν 3 (748, 194)] were obtained for Cu(pmed)Br 2 and Cu(pemed)Br 2 , respectively. In addition, intense absorption bands were observed in the ~285 nm region for both two complexes, and these were assigned to intraligand transitions (π-π*). The blue shift (16 nm) in the wavelength of Cu(pmed)Br 2 as compared to Cu(pemed)Br 2 indicates that coordination geometry in the N -alkylated complex is less distorted than that in the non- N -alkylated complex, which may be due to the ligand field strength imparted by the nitrogen donor atoms.
PPT Slide
Lager Image
Electronic absorption spectra and transition analysis spectra by Gaussian resolution of Cu(pmed)Br2 (a) and Cu(dpmed)Br2 (b).
Hydrogen bonds for Cu(pmed)Br2[Å ando]
PPT Slide
Lager Image
Symmetry code: (i) x, y+1, z (ii) −x+1, −y, −z+2
X-band EPR spectra were recorded in the solid-state and in frozen glass samples (toluene/methanol, 50/50% by volume at 77 K). The data are summarized in Table 3 . The powdered EPR line shape of Cu(pmed)Br 2 showed an isotropic broad singlet with = 2.808 at 77 K, which resolved into parallel (g ) and perpendicular (g⊥) components of g = 2.260 and g⊥ = 2.060 in frozen glass at 77 K. Lack of hyperfine structure in solid state was probably due to intermolecular hydrogen bonding between the H(11) atom and the adjacent terminal bromide Br(2). On the other hand, Cu(pemed)Br 2 exhibited three well resolved g-values of g xx = 2.046, g yy = 2.089 and g zz = 2.191 in the solid state at 77 K and well defined hyperfine splitting with g = 2.286 and g⊥ = 2.072 in solution EPR spectra at 77 K. The EPR spectral feature of g > g⊥ > 2.0023 in both complexes is consistent with a pentacoordinated square pyramidal structure with unpaired electrons in a d x2-y2 orbital. Figure 5 shows EPR spectra of Cu(pemed)Br 2 both in powder and frozen solution at 77 K.
PPT Slide
Lager Image
X-band EPR spectra of Cu(dpmed)Br2 in powder (a) and frozen solution (b) at 77 K.
PPT Slide
Lager Image
The plots of magnetic susceptibilities χm and 1/χm vs. temperature at 4-300 K for Cu(dpmed)Br2. Calculated (—) and experimental (●) magnetic data are shown.
The molar magnetic susceptibilities of powdered samples were measured as a function of temperature in the range 4 K to 300 K and shown in Figure 6 . Magnetic susceptibility increased as temperature decreased and no maximum susceptibility was observed, which is in keeping with paramagnetic behavior. In fact, magnetic susceptibility data well fitted Curie-Weiss law, χ m = C/(T − θ), indicating no magnetic interactions between copper(II) ions. A linear regression of χ m vs T results Curie-Weiss temperature of θ = 0.23 K and a Curie constant of C = 0.31 cm3 Kmol -1 for Cu(pmed)Br 2 , and θ = 0.13 K and C = 0.42 cm 3 Kmol -1 for Cu(pemed)Br 2 . The calculated intermolecular separations of Cu…Cu and Br1…Br1 were 6.635 Å and 4.594 Å for Cu(pmed)Br 2 , and 7.029 Å and 4.625 Å for Cu(pemed)Br2, which were too great to enable magnetic exchange between copper(II) ions. 46 The calculated effective magnetic moments from the equation, μ eff = 2.828(χ m × T) 1/2 were 1.96 B.M. and 1.92 B.M. for Cu(pmed)Br 2 and Cu(dpmed)Br 2 , respectively.
Five-coordinated copper(II) bromide complexes, Cu(pmed)Br 2 and Cu(dpmed)Br 2 , with tridentate Schiff base containing amine and pyridine moiety, were prepared from the ligands and copper(II) bromide. The copper(II) center of Cu(pmed)Br 2 features a distorted square pyramidal coordination geometry with two Br atoms and the three N atoms of the tridentate ligand. Hydrogen bonds formed between the amine hydrogen atoms and apical Br atoms of neighbouring molecules resulted in the formation of two-dimensional networks in the ab plane. On the other hand, Cu(dpmed)Br 2 has an almost square pyramidal geometry and monomeric molecules are stabilized through intermolecular π-π interactions between the pyridine rings. In both compounds, no magnetic interactions occur between the copper(II) metal ions because the Cu-Cu distances are too far for magnetic contact.
This work was supported by Basic Science Research Program through the National Research Foundation of Korea (NRF) funded by the Ministry of Education, Science and Technology (No. 20110003799).
Sain S. , Saha R. , Mostafa G. , Fleck M. , Bandyopadhyay D. 2012 Polyhedron 31 82 -    DOI : 10.1016/j.poly.2011.08.040
Naiya S. , Biswas C. , Drew M. G. B. , Gomez-Garcia C. J. , Clemente-Juan J. M. , Ghosh A. 2010 Inorg. Chem. 49 6616 -    DOI : 10.1021/ic1005456
Franks M. , Gadzhieva A. , Ghandhi L. , Murrell D. , Blake A. J. , Davies E. S. , Lewis W. , Moro F. , McMaster J. , Schroder M. 2013 Inorg. Chem. 52 660 -    DOI : 10.1021/ic301731w
Meghdadi S. , Mereiter K. , Langer V. , Amiri A. , Erami R. S. , Massoud A. A. , Amirnasr M. 2012 Inorg. Chim. Acta 385 31 -    DOI : 10.1016/j.ica.2011.12.025
Zabierowski P. , Szklarzewicz J. , Kurpiewska K. , Lewinski K. , Nitek W. 2013 Polyhedron 49 74 -    DOI : 10.1016/j.poly.2012.09.029
Goswami T. K. , Chakravarthi B. V. S. K. , Roy M. , Karande A. A. , Chakravarty A. R. 2011 Inorg. Chem. 50 8452 -    DOI : 10.1021/ic201028e
Tandon S. S. , Bunge S. D. , Sanchiz J. , Thompson L. K. 2012 Inorg. Chem. 51 3270 -    DOI : 10.1021/ic202732k
Gungor E. , Kara H. 2012 Inorg. Chim. Acta 384 137 -    DOI : 10.1016/j.ica.2011.11.047
Hamid M. H. S. A. , Ali M. A. , Mirza A. H. , Bernhardt P. V. , Moubaraki B. , Murray K. S. 2009 Inorg. Chim. Acta 362 3648 -    DOI : 10.1016/j.ica.2009.04.019
Sasmal S. , Sarkar S. , Aliaga-Alcalde N. , Mohanta S. 2011 Inorg. Chem. 50 5687 -    DOI : 10.1021/ic200462g
Dhar S. , Nethaji M. , Chakravarty A. R. 2005 Inorg. Chim. Acta 358 2437 -    DOI : 10.1016/j.ica.2005.02.006
Bhar K. , Choubey S. , Mitra P. , Rosair G. , Ribas J. , Ghosh B. K. 2011 J. Mol. Struct. 988 128 -    DOI : 10.1016/j.molstruc.2010.12.042
Adhikary C. , Mal D. , Okamoto K.-I. , Chaudhuri S. , Koner S. 2006 Polyhedron 25 2191 -    DOI : 10.1016/j.poly.2006.01.011
Sain S. , Saha R. , Mostafa G. , Fleck M. , Bandyopadhyay D. 2012 Polyhedron 31 82 -    DOI : 10.1016/j.poly.2011.08.040
Liu H. , Gao F. , Niu D. , Tian J. 2009 Inorg. Chim. Acta 362 4179 -    DOI : 10.1016/j.ica.2009.06.021
Blomenkemper M. , Schroder H. , Pape T. , Hahn F. E. 2012 Inorg. Chim. Acta 390 143 -    DOI : 10.1016/j.ica.2012.04.023
Li R. , Moubaraki B. , Murray K. S. , Brooker S. 2008 J. Chem. Soc., Dalton Trans. 6014 -
Kolks G. , Waszczak J. V. 1980 J . Am. Chem. Soc. 102 4832 -    DOI : 10.1021/ja00534a045
Harris S. A. , Ciszewski J. T. , Odom A. L. 2001 Inorg. Chem. 40 1987 -    DOI : 10.1021/ic001238r
Katayev E. , Li Y. , Odom A. L. 2002 Chem. Commun. 838 -
Alves W. A. , Filho S. A. D. A. , Santos R. H. D. A. , Ferreira A. M. D. C. 2003 Inorg. Chem. Commun. 6 294 -    DOI : 10.1016/S1387-7003(02)00757-8
Naskar S. , Naskar S. , Mayer-Figge H. , Sheldrick W. S. , Corbella M. , Tercero J. , Chattopadhyay S. K. 2012 Polyhedron 35 77 -    DOI : 10.1016/j.poly.2011.12.042
Mandal S. , Lloret F. , Mukherjee R. 2009 Inorg. Chim. Acta 362 27 -    DOI : 10.1016/j.ica.2008.02.072
Lee H. W. , Sengottuvelan N. , Seo H.-J. , Choi J. S. , Kang S. K. , Kim Y.-I. 2008 Bull. Korean Chem. Soc. 29 1711 -    DOI : 10.5012/bkcs.2008.29.9.1711
Lee H.-W. , Kim H.-J. , Kang S. K. , Heo J. Y. , Kim Y.-I. 2007 Bull. Korean Chem. Soc. 28 855 -    DOI : 10.5012/bkcs.2007.28.5.855
Kim Y.-I. , Lee Y.-S. , Seo H.-J. , Lee J.-Y. , Kang S. K. 2007 Acta Cryst. E63 m2810 -
Kim Y.-I. , Lee Y.-S. , Seo H.-J. , Nam K.-S. , Kang S. K. 2008 Acta Cryst. E64 m358 -
Kim Y.-I. , Seo H.-J. , Kim J.-H. , Lee Y.-S. , Kang S. K. 2010 Acta Cryst. E66 m124 -
Sheldrick G. M. 2008 Acta Cryst. A64 112 -
Addison A. W. , Rao T. N. , Reedijk J. , Van Rijn J. , Verschoor G. C. 1984 J. Chem. Soc. Dalton Trans. 1349 -
Tyagi S. , Hathaway B. J. , Kramer S. , Stratemeier H. , Reinen D. 1984 J. Chem. Soc. Dalton Trans. 2087 -
Mohamadou A. , Moreau J. , Dupont L. , Wenger E. 2012 Inorg. Chim. Acta 383 267 -    DOI : 10.1016/j.ica.2011.11.016
Tounsi N. , Dupont L. , Mohamadou A. , Guillon E. , Aplincourt M. , Rogez G. 2008 Polyhedron 27 3674 -    DOI : 10.1016/j.poly.2008.09.020
Banerjee S. , Gangopadhyay J. , Lu C.-Z. , Chen J.-T. , Ghosh A. 2004 Eur. J. Inorg. Chem. 2533 -
Calligaris M. , Randaccio L. , Gillard R. O. , McCleverty J. 1987 2 724 -
Ali M. A. , Mirza A. H. , Ravoof T. B. S. A. , Bernhardt P. V. 2004 Polyhedron 23 2031 -    DOI : 10.1016/j.poly.2004.05.007
Tuna F. , Pascu G. I. , Sutter J.-P. , Andruh M. , Golhen S. , Guillevic J. , Pritzkow H. 2003 Inorg. Chim. Acta 342 131 -    DOI : 10.1016/S0020-1693(02)01155-6
Shaabani B. , Khandar A. A. , Dusek M. , Pojarova M. , Mahmoudi F. 2013 Inorg. Chim. Acta 394 563 -    DOI : 10.1016/j.ica.2012.08.027
Ali M. A. , Mirza A. H. , Bujang F. H. , Hamid M. H. S. A. , Bernhardt P. V. 2006 Polyhedron 25 3245 -    DOI : 10.1016/j.poly.2006.05.027
Karmakar R. , Choudhury C. R. , Hughes D. L. , Yap G. P. A. , Fallah M. S. E. , Desplanches C. , Sutter J.-P. , Mitra S. 2006 Inorg. Chim. Acta 359 1184 -    DOI : 10.1016/j.ica.2005.09.013
Billington D. C. , Lowe P. R. , Rathbone D. L. , Schwalbe C. H. 2000 Acta Cryst. C56 e211 -
Mukherjee P. , Drew M. G. B. , Ghosh A. 2008 Eur. J. Inorg. Chem. 3372 -
Sarkar B. , Drew M. G. B. , Estrader M. , Diaz C. , Ghosh A. 2008 Polyhedron 27 2625 -    DOI : 10.1016/j.poly.2008.05.004
McLachlan G. A. , Fallon G. D. , Martin R. L. , Spiccia L. 1995 Inorg. Chem. 34 254 -    DOI : 10.1021/ic00105a041
Patel R. N. , Singh N. , Gundla V. L. N. 2006 Polyhedron 25 3312 -    DOI : 10.1016/j.poly.2006.06.017
Lee Y.-M. , Park S.-M. , Kang S. K. , Kim Y.-I. , Choi S.-N. 2004 Bull. Korean Chem. Soc. 25 823 -    DOI : 10.5012/bkcs.2004.25.6.823