Synthesis, Structure, and Physical Properties of a Barium Complex with 5-Sulfoisophthalic Acid Sodium Salt

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DOI: 10.1002/zaac.201000371

Synthesis, Structure, and Physical Properties of a Barium Complex with 5-Sulfoisophthalic Acid Sodium Salt

Gang Wu,[a] Fun-Jun Yin,[b] Hao Wei,[a] Zhen-Feng Liu,[a] and Xiao-Feng Wang*[c]

Keywords: Barium; Coordination modes; Sulfonates; Carboxylates; 5-Sulfoisophthalic acid

Abstract. The complex [Ba3(sip)2(H2O)9]·H2O (1) (NaH2sip = 5-sul-foisophthalic acid sodium) was synthesized and characterized by sin-gle-crystal X-ray diffraction. Structural determination reveals that theasymmetric unit in 1 contains two crystallographically independentBaII atoms. The Ba1 atom is eight-coordinate with distorted mono-capped pentagonal bipyramidal arrangement, whereas the Ba2 atom isten-coordinated with bicapped tetragonal prismatic arrangement. Thetwo carboxylate groups of sip3– adopt different coordination modes,

Introduction

The rational design and construction of coordination poly-mers based upon assembly of metal ions and multifunctionalorganic ligands is an interesting research field, not only be-cause of their intriguing structural topologies but also due totheir potential application as functional materials.[1–6] In thelast few years, much progress has been made on the designand synthesis of novel coordination frameworks and the rela-tionships between their structures and properties.[7–10] An ef-fective and facile approach for the synthesis of such complexesis still the appropriate choice of well-designed organic ligandsas bridges or terminal groups with metal ions or metal clustersas nodes.[11,12]

However, one of the challenges is the rational and controlla-ble preparation of metal-organic frameworks. The formation isgreatly affected by the organic ligands, the nature of the metalions, the counterions, and other factors. In the past ten years,the studies of solid-state metal-organic coordination networksconcentrated on transition metal complexes, little attention waspaid to the systematic study of the equivalent behavior of s-block metals.[13–15] The formation of metal-organic frame-works (MOFs) with alkaline earth metal ions has not been

* Prof. Dr. X.-F. WangFax: +86-25-86178274E-Mail: [email protected]

[a] Department of Chemistry and Life and ScienceChu Zhou UniversityAn Hui ProvinceChu Zhou, 239012, P. R. China

[b] Jiangsu Marine Resources Development Research InstituteHuaihai Institute of TechnologyLianyungang, 222005, Jiangsu, P. R. China

[c] Biochemistry & Environment Engineering CollegeXiao Zhuang UniversityNanjing 211171, P. R. China

596 © 2011 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim Z. Anorg. Allg. Chem. 2011, 637, 596–601

μ2-η1:η1-bridging, and μ2-η2:η1-bridging. The sulfonate group coordi-nates to three different BaII atoms in a tridentate μ3 mode to generatea ladder-like one-dimensional chain. The chains are connected by μ2-η1:η1-bridging carboxylate groups to form a wave-like two-dimen-sional network, which are further linked by sip3– anions to generate athree-dimensional structure. The thermal stability and luminescenceproperties of complex 1 were also investigated.

widely investigated,[15,16] even though many of these materialsare already of commercial importance.[17] Because of the largeradius of alkaline earth metals, such as calcium, strontium, ba-rium, these metal ions have large coordination numbers com-pared to transition metal ions. Alkaline earth metals have sev-eral advantages for application in materials science; they arenontoxic, cheap, and generally amenable to aqueous prepara-tion. Some alkaline earth complexes were found to exhibit in-teresting properties. For example, one-dimensional[Ca(diglyme)2(H2O)2]I2, which crystallizes in the polar spacegroup Cc, has non-linear optical (NLO) and piezoelectricproperties.[18,19] The mixed-metal networks of{Ba2(H2O)4[LnL3(H2O)2](H2O)nCl}∞, Ln = Sm3+ (1), Eu3+ (2),Gd3+ (3), Tb3+ (4), Dy3+ (5) contain open channels, whichreadily absorb and desorb water accompanied by a sponge-likeshrinkage and expansion of the host. CO2 sorption measure-ments confirmed microporosity with a DR surface area of718 m2·gm–1 and an average pore size of 6.4 Å.[20]These observations sparked the recent interest in the chemis-try of alkaline earth metal complexes.[21,22] Kennedy et al. syn-thesized and analyzed the crystal structures of alkaline earthmetal salts of simple sulfonated azo dyes.[23,24] Using nitrogen-containing ligands, low-dimensional coordination polymers ofalkaline earth metal salts, in most cases by bridging halides,were generated by Skelton and White et al.[25–27] Zhu et al.synthesized layered structures of [Ca3(bta)2(H2O)8]·3H2O and[Ba3(bta)2(H2O)8] by using flexible 1,3,5-triacetic acid (H3bta)as ligand, in which each bta3– ligand coordinates to Ca2+ orBa2+ ions through two of its three carboxylate groups, whichadopt different coordination modes.[28] Organic ligands withcarboxylate functions are of research interest because they areable to adopt a variety of coordination modes and result indiverse multidimensional architectures.[5,29–33] Particularly,most of the reported work was devoted to organic aromatic

A Barium Complex with 5-Sulfoisophthalic Acid Sodium Salt

polycarboxylate ligands, especially 1,4-benzenedicarboxylate,1,3,5-benzenetricarboxylate, and 1,2,4,5-benzenetetra-carboxylate.[34,35] Little attention has been paid on sulfonate-containing ligands. Considering the diverse coordinationmodes of sulfonates[1,36–41] and radii and coordination numbersof calcium(II), strontium(II), and barium(II), complexes withsulfonate-containing ligands and alkaline earth metals with at-tractive structures and properties may be obtained.Recenty, we synthesized two isostructural complexes[Ca(hssal)(H2O)2]n and [Sr(hssal)(H2O)2]n (hssal2– = 5-sulfo-salicylate) with two-dimensional network structure by usingthe ligand 5-sulfosalicylic acid and alkaline earth metal saltsunder hydrothermal conditions. Luminescence properties andthermal stabilities of both complexes were investigated.[42] Inthis manuscript, we describe the syntheses, structure, and prop-erties of the coordination polymer [Ba3(sip)2(H2O)9]·H2O (1)with the ligand 5-sulfoisophthalic acid sodium salt (NaH2sip)synthesized under hydrothermal conditions.

Experimental Section

General Methods

All reagents commercially available were of reagent grade and usedwithout further purification. Solvents were purified according to stand-ard methods. C, H, and S elemental analyses were carried out with aPerkin–Elmer 240C elemental analyzer. IR spectra were recorded witha Nicolet 6700 FT-IR spectrophotometer by using KBr pellet in therange 4000–400 cm–1. Thermal properties of [Ba3(sip)2(H2O)9]·H2O(1) were analyzed by TGA under 100.0 mL·min–1 nitrogen flow rate,while the temperature was increased at a rate of 20.00 °C·min–1 from28 to 1200 °C. Luminescence spectra for the solid samples were re-corded at room temperature with an Aminco Bowman Series 2 spectro-photometer with a xenon arc lamp as the light source. In the measure-ments of the emission and excitation spectra, the pass width is 5.0 nm.Powder X-ray diffraction patterns were performed with a Bruker D8ADVANCE X-ray diffractometer with Cu-Kα1 radiation at 40 kV and40 mA.

X-ray Crystallographic Studies

A crystal of the title compound with dimensions0.20 mm × 0.15 mm × 0.20 mm was selected for diffraction analysis.The X-ray diffraction intensity data were collected with a Bruker SmartApex II CCD diffractometer equipped with a graphite-monochromatedMo-Kα (λ = 0.71073 Å) radiation at 296(2) K. The structure wassolved by direct methods with SHELX97. All non-hydrogen atomswere located with successive difference Fourier syntheses. All atomiccoordinates and anisotropic thermal parameters of non-hydrogen atomsas well as equivalent isotropic thermal parameters of hydrogen atomswere refined by full-matrix least-squares techniques on F2. Details ofthe crystal parameters, data collection, and refinement for complex 1are summarized in Table 1. Selected bond lengths and bond angles arelisted in Table 2.

Z. Anorg. Allg. Chem. 2011, 596–601 © 2011 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim www.zaac.wiley-vch.de 597

Table 1. Crystallographic data for complex 1.

Empirical formula C16H16O24S2Ba3Fw 1068.42Crystal system OrthorhombicSpace group Pbcaa /Å 14.966(3)b /Å 7.4087(18)c /Å 26.828(6)α /deg 90.00β /deg 90.00γ /deg 90.00V /Å3 2974.6(12)Z 4Crystal size /mm 0.20 × 0.15 × 0.20Dc /g·cm–3 2.386μ /mm–1 4.167Independent reflections 3355Observed reflections 2650Rint 0.0364Goodness of fit 1.066Ra)/wRb) 0.0282 / 0.0583

a) R = Σ ||Fo|–|Fc||/Σ|Fo|. b) wR = |Σw(|Fo|2–|Fc|2)|/Σ|w(Fo)2|1/2, wherew = 1/[σ2(Fo2) + (aP)2 + bP]. P = (Fo2 + 2Fc2)/3.

CCDC-739361 contains the supplementary crystallographic data forthe structure in this paper. This data can be obtained free of chargevia http://www.ccdc.cam.ac.uk/conts/ retrieving.html, or from theCambridge Crystallographic Data Centre, CCDC, 12 Union Road,Cambridge CB2 1EZ, UK; Fax: 44-1223-336-033; or E-Mail:[email protected].

Preparation of [Ba3(sip)2(H2O)9]·H2O (1): A mixture of 5-sulfoi-sophthalic acid sodium salt (NaH2sip: C8H5NaO7S, 26.8 mg,0.1 mmol) and BaCO3 (19.7 mg, 0.1 mmol) in distilled water (8 mL)was stirred at room temperature for 10 min. Afterwards, CH3OH(3 mL) was added to the clear solution and sealed in a 25 mL Teflon-lined stainless steel container, which was heated at 150 °C for 3 days.After the sample was cooled to room temperature, colorless rod crys-tals were obtained (Yield 18.2 mg). C16H26O24S2Ba3 (1078.48): calcd.C 17.82; H 2.43; S 5.95 %; found: C 17.91; H 2.52; S 6.01 %. IR(KBr): ν̃ = 3446 (bs), 1639 (s), 1391 (s), 1235 (m), 1190 (m), 1104(w), 1052 (m), 754 (m) cm–1.

Results and DiscussionIn the IR spectrum of 1, a signal at 3446 cm–1 suggests thepresence of lattice water or coordinated water molecules. Astrong band at 1639 cm–1 is in agreement with the presence ofcarboxylate functions. Complex 1 is stable in air and crystalli-zes in the orthorhombic space group Pbca. X-ray crystallogra-phy shows that 1 has a three-dimensional polymeric structure.Selected bond lengths and angles for 1 are listed in Table 2.In complex 1, the asymmetric unit contains two crystallo-

graphically independent barium atoms (Figure 1) with differ-ent coordination environments. The Ba1 atom is eight-coordi-nate with an O8 donor set: three oxygen atoms (O3, O4, O6)from three different carboxylate groups of three sip3– ligands,one oxygen atom of the carboxylate groups adopting a μ2-bridging mode coordinates to Ba1 and Ba2, two oxygen atoms(O1A, O10) from two different sulfonate ligand groups, threeoxygen atoms (O2, O5, and O8) from three water molecules

G. Wu, F.-J. Yin, H. Wei, Z.-F. Liu, X.-F. WangARTICLE

Table 2. Selected bond lengths /Å and angles /° for complex 1.

O1–Ba1#1 2.803(3) Ba1–O1#2 2.803(3)Ba1–O2 2.759(4) Ba1–O3 2.763(3)Ba1–O4 2.729(3) Ba1–O5 2.859(3)Ba1–O6 2.876(3) Ba1–O8 2.909(3)Ba1–O10 2.722(3) Ba2–O9#3 2.776(3)Ba2–O9 2.776(3) Ba2–O4 3.059(3)Ba2–O11#3 2.864(4) Ba2–O7 2.872(3)Ba2–O7#3 2.872(3) Ba2–O5#3 2.940(3)Ba2–O5 2.940(3) Ba2–O4#3 3.059(3)O10–Ba1–O4 73.90(9) O10–Ba1–O2 93.12(11)O4–Ba1–O2 87.89(9) O10–Ba1–O3 149.88(9)O4–Ba1–O3 135.93(9) O2–Ba1–O3 85.43(10)O10–Ba1–O1#2 139.79(8) O4–Ba1–O1#2 67.71(8)O2–Ba1–O1#2 74.31(10) O3–Ba1–O1#2 68.54(8)O10–Ba1–O5 110.87(11) O4–Ba1–O5 75.56(9)O2–Ba1–O5 145.06(12) O3–Ba1–O5 85.63(10)O1–Ba1–O5#2 70.97(10) O10–Ba1–O6 71.82(9)O4–Ba1–O6 140.97(9) O2–Ba1–O6 75.99(10)O3–Ba1–O6 78.68(9) O1–Ba1–O6#2 136.92(8)O5–Ba1–O6 134.63(8) O10–Ba1–O8 94.45(9)O4–Ba1–O8 131.90(8) O2–Ba1–O8 139.98(9)O3–Ba1–O8 69.01(9) O1–Ba1–O8#2 119.93(9)O5–Ba1–O8 65.31(9) O6–Ba1–O8 69.32(8)O9–Ba2–O9#3 180.000(1) #3O9–Ba2–O11#3 85.78(10)O9–Ba2–O11#3 94.22(10) O9–Ba2–O7#3 82.86(8)O9–Ba2–O7 97.14(8) O11–Ba2–O7#3 112.61(10)#3O9–Ba2–O7#3 97.14(8) O9–Ba2–O7#3 82.86(8)#3O11–Ba2–O7#3 67.39(10) O7–Ba2–O7#3 180.0#3O9–Ba2–O5#3 113.60(8) O9–Ba2–O5#3 66.40(8)#3O11–Ba2–O5#3 61.58(12) O7–Ba2–O5#3 63.56(9)#3O7–Ba2–O5#3 116.44(10) O9–Ba2–O5#3 66.40(8)O9–Ba2–O5 113.60(8) O11–Ba2–O5#3 118.42(12)O7–Ba2–O5 116.44(10) O7–Ba2–O5#3 63.56(9)O5–Ba2–O5#3 180.00(9) #3O9–Ba2–O4#3 44.31(7)O9–Ba2–O4#3 135.69(7) #3O11–Ba2–O4#3 59.60(10)O7–Ba2–O4#3 66.89(8) #3O7–Ba2–O4#3 113.11(8)#3O5–Ba2–O4#3 69.58(8) O5–Ba2–O4#3 110.42(8)O9–Ba2–O4#3 135.69(7) O9–Ba2–O4 44.31(7)O11–Ba2–O4#3 120.40(10) O7–Ba2–O4 113.11(8)O7–Ba2–O4#3 66.89(8) O5–Ba2–O4#3 110.42(8)O5–Ba2–O4 69.58(8) O4–Ba2–O4#3 180.00(5)

Symmetry transformations are used to generate equivalent atoms: #1: x, 1 + y, z; #2: x, –1 + y, z; #3: 1 – x, –y, 1 – z.

for Ba1, one oxygen atom (O5) of among the water moleculesadopts a μ2-bridging coordination mode to connect Ba1 andBa2. The coordination environment around Ba1 is best de-scribed as distorted capped pentagonal bipyramidal. The oxy-gen atoms O2, O4, O5, O6, and O8 are located in the pentago-nal plane. O10 and O3 occupy the apical positions with a Ba1–O bond length of 2.6820(19) Å and a trans angle of163.06(10)° (Table 2).The Ba2 atom is ten-coordinated with an O10 donor set: fouroxygen atoms from two different carboxylate groups of differ-ent two sip3– ligands that adopt μ2-η2:η1-bridging (one oxygenatom connects two metal ions, the other connects one metalatom, and the carboxylic group coordinates to two metal at-oms) coordination modes (Scheme 1), but chelate with the Ba2atom, two oxygen atoms from sulfonate groups, four oxygenatoms from water molecules, two of them take a μ2-bridgingmode to coordinate to Ba1 and Ba2. The Ba2–O bond lengthsare in the range 2.776(3)–3.059(3) Å, and the arrangement

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around the Ba2 atom is approximately bicapped tetragonalprismatic, in which the oxygen atoms O5, O7, O9, and O11form the top plane, and the oxygen atoms O5A, O7A, O9A,and O11A are localized in the bottom plane, whereas O4 andO4A make up the two opposite tetragonal side faces.Each oxygen atom of the sulfonate function coordinates toone BaII atom. Therefore, the sulfonate group takes a tridentateμ3-coordination mode. However, the carboxylate functions ofthe ligand sip3– adopt two different coordination modes in 1,as schematically shown in Scheme 1, μ2-η2:η1-bridging (eachoxygen atom coordinates to one metal atom, and the carboxyl-ate group coordinates to two metal atoms) and μ2-bridging(Scheme 1).If the coordination mode of sulfonate group only is consid-ered, an infinite one-dimensional (1D) chain is formed (Fig-ure 2). In this chain, the sulfonate groups adopt a μ3-bridgingcoordination mode by two oxygen atoms from two sip3– li-gands to generate a wavelike 1D chain [the angles of Ba2A–


Figure 1. ORTEP view of the coordination environment of the BaIIatoms in 1 with 50 % probability displacement. Hydrogen atoms areomitted for clarity. O6A (–x + 3/2, y – 1/2, z), O4A, O5A, O7A, O9A,O11A (–x + 3/2, –y, z + 3/2), O7B (–x + 3/2, –y + 1, z + 3/2), O1A(x, y – 1, z).

Scheme 1. Coordination mode of sip3–.

Figure 2. Infinite 1D helix channel structure in 1.


Ba1–Ba2 and Ba1–Ba2–Ba2B are 135.345(9) and 120.252(7)°,respectively]. The corresponding Ba2–O3A bond length is2.786(2) Å, and the Ba2–O3A–Ba2B bond angle is 105.22(7)°.The distances between Ba1–Ba2, Ba2–Ba3, and Ba1–Ba5 are4.651, 7.607, 7.409 Å, respectively, which are larger than thesum of the van der Waals radii (4.28 Å). In this chain, the BaII

atoms and μ3-bridging sulfonate groups form an infinite one-dimensional (1D) chain through sharing side circles consistingof four sulfonate groups and four BaII atoms.If we neglect the linkage of the ligand sip3–, a two dimen-sional (2D) wave-like network is obtained (Figure 3 a,b). Theμ2-bridging carboxylate groups link these 1D chains to gener-ate a wave-like 2D network (Figure 3 a,b) because the O–C–Oangle of carboxylate group is 124.3° and takes trans coordina-tion mode. The 2D networks are further linked together by thebenzene rings to give a 3D coordination polymer (Figure 4).

Figure 3. Wave-like 2D network structure in 1. Hydrogen atoms andwater molecules are omitted for clarity. Side (left, a) and top (right, b)views of 2D network structure in 1.

Figure 4. Crystal packing diagram for 1. Hydrogen atoms and watermolecules are omitted for clarity.

G. Wu, F.-J. Yin, H. Wei, Z.-F. Liu, X.-F. WangARTICLE

Thermal Stability Analysis

To examine the thermal stability of complex 1, thermo gravi-metric (TG) analyses were carried out under a nitrogen flowrate of 100.0 mL·min–1 and a temperature increase from 28 to1000 °C at a rate of 20.00 °C·min–1. The TG curve of 1 isshown in Figure 5. A total weight loss of 46.78 % is observedin the temperature range 28–1000 °C. The TG curve of 1 ex-hibits two weight loss stages between 36–253 °C (16.60 %)and 253–970 °C. The first weight loss corresponds to the re-lease of coordinated and lattice water molecules (calcd.16.87 %). The second weight loss between 253–970 °C of ca.30.18 % corresponds to the loss of benzene and carbon dioxide(calcd. 31.09 %). The residue may be the mixture of bariumoxide and barium sulfate.

Figure 5. TG curve of 1.

Furthermore, dehydration and rehydration experiments wereperformed for 1 and powder X-ray diffraction (PXRD) wasused to check the phases. 1 was heated at 250 °C for 24 hours,to obtain complete loss of water. The powdered dehydratedphase has a PXRD pattern different from complex 1 (Fig-

Figure 6. Powder X-ray diffraction patterns of 1. The dehydrated, rehy-drated, and simulated phase are based on the single-crystal structure of 1.

600 www.zaac.wiley-vch.de © 2011 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim Z. Anorg. Allg. Chem. 2011, 596–601

ure 6), which indicates that the porous framework probablyshrank after removal of water. The dehydrated phase was after-wards exposed to water vapor at room temperature for another24 hours. However, the rehydrated sample has a PXRD patterncompletely different from that of 1, which shows that the dehy-dration and rehydration processes for 1 are irreversible.

Luminescence Properties of Complex 1

The luminescent behavior of complex 1 was investigated atroom temperature in the solid state. The emission spectrum isshown in Figure 7. Complex 1 exhibits a luminescence emis-sion at 411 nm upon excitation at 340 nm, which is similar tothat of the ligand under the same excitation wavelength. Theobserved emission of complex 1 is probably due to π–π* intra-ligand fluorescence since a similar emission was also observedfor the ligand itself.

Figure 7. Solid state fluorescence spectrum of 1 at room temperature.

ConclusionsComplex 1 was obtained by a hydrothermal process. In the

ligand sip3–, the two carboxylate functions adopt different co-ordination modes, μ2-η1:η1-bridging mode and μ2-η2:η1-bridg-ing. The sulfonate group takes a tridentate μ3-coordinationmode to coordinate to three different BaII atoms, each oxygenatom adopts a monodentate coordination mode. The sulfonategroups link the BaII atoms to generate a ladder-like one-dimen-sional chain, which are further connected by μ2-η1:η1-bridgingcarboxylate functions to form wave-like two-dimensional net-works. These two-dimensional networks are further linked bybenzene rings to generate a three-dimensional structure. Thethermal stability and luminescence properties of complex 1 areinvestigated.

AcknowledgementThe authors are grateful to the University Science Foundation of AnHui Education Department (Grant No. KJ2009B104) and The Applied


Chemistry Key Subject of An Hui Provience (No. 200802187C) forfinancial support of this work.

References[1] S. R. Fan, L. G. Zhu, Inorg. Chem. 2006, 45, 7935.[2] Y. W. Li, R. T. Yang, J. Am. Chem. Soc. 2006, 128, 726.[3] X. M. Gao, D. S. Li, J. J. Wang, F. Fu, Y. P. Wu, H. M. Hu, J. W.

Wang, CrystEngComm 2008, 10, 479.[4] X. N. Chen, W. X. Zhang, X. M. Chen, J. Am. Chem. Soc. 2007,

129, 15738.[5] C. S. Liu, J. J. Wang, L. F. Yan, Z. Chang, X. H. Bu, E. C. Sañ-

uso, J. Ribas, Inorg. Chem. 2007, 46, 6299.[6] W. T. Chen, M. S. Wang, X. Liu, G. C. Guo, J. S. Huang, Cryst.

Growth Des. 2006, 6, 2289.[7] C. D. Wu, W. B. Lin, Angew. Chem. Int. Ed. 2007, 46, 1075.[8] J. M. Taylor, A. H. Mahmoudkhani, G. K. H. Shimizu, Angew.

Chem. Int. Ed. 2007, 46, 795.[9] M. Dan, C. N. R. Rao, Angew. Chem. Int. Ed. 2006, 45, 281.[10] P. Jensen, D. J. Price, S. R. Batten, B. Moubaraki, K. S. Murray,

Chem. Eur. J. 2000, 6, 3186.[11] J. P. Zhang, Y. Y. Lin, X. C. Huang, X. M. Chen, J. Am. Chem.

Soc. 2005, 127, 5495.[12] L. F. Ma, L. Y. Wang, D. H. Lu, S. R. Batten, J. G. Wang, Cryst.

Growth Des. 2009, 9, 1741.[13] P. C. Andrikopoulos, D. R. Armstrong, E. Hevia, A. R. Kennedy,

R. E. Mulvey, C. T. O’Hara, Chem. Commun. 2005, 1131.[14] H. Bock, J. M. Lehn, J. Pauls, S. Holl, V. Krenzel, Angew. Chem.

Int. Ed. 1999, 38, 952.[15] K. W. Henderson, A. R. Kennedy, L. Macdonald, D. J. Mac-

Dougall, Inorg. Chem. 2003, 42, 2839.[16] K. M. Fromm, Coord. Chem. Rev. 2008, 252, 856.[17] A. R. Kennedy, J. B. A. Kirkhouse, L. Whyte, Inorg. Chem.

2006, 45, 2965.[18] K. M. Fromm, Chem. Eur. J. 2001, 7, 2236.[19] K. M. Fromm, E. D. Gueneau, A. Y. Robin, W. Maudez, J. Sague,

R. Bergougnant, Z. Anorg. Allg. Chem. 2005, 631, 1725.[20] B. D. Chandler, D. T. Cramb, G. K. H. Shimizu, J. Am. Chem.

Soc. 2006, 128, 10403.


[21] U. Englich, K. Ruhlandt-Senge, Coord. Chem. Rev. 2000, 210,135.

[22] T. P. Hanusa, Coord. Chem. Rev. 2000, 210, 329.[23] A. R. Kennedy, M. P. Hughes, M. L. Monaghan, E. Staunton,

S. J. Teat, W. E. Smith, J. Chem. Soc. Dalton Trans. 2001, 2199.[24] A. R. Kennedy, J. B. A. Kirkhouse, K. M. McCarney, O. Puisse-

gur, W. E. Smith, E. Staunton, S. J. Teat, J. C. Cherryman, R.James, Chem. Eur. J. 2004, 10, 4606.

[25] A. F. Waters, A. H. White, Aust. J. Chem. 1996, 49, 27.[26] D. L. Kepert, B. W. Skelton, A. F. Waters, A. H. White, Aust. J.

Chem. 1996, 49, 47.[27] B. W. Skelton, A. F. Waters, A. H. White, Aust. J. Chem. 1996,

49, 99.[28] H. F. Zhu, Z. H. Zhang, W. Y. Sun, T. Okamura, N. Ueyama,

Cryst. Growth Des. 2005, 5, 177.[29] X. J. Gu, D. F. Xue, CrystEngComm 2007, 9, 471.[30] L. F. Ma, L. Y. Wang, Y. Y. Wang, S. R. Batten, J. G. Wang, In-

org. Chem. 2009, 48, 915.[31] D. R. Xiao, E. B. Wang, H. Y. An, Z. M. Su, Y. G. Li, L. Gao,

C. Y. Sun, L. Xu, Chem. Eur. J. 2005, 11, 6673.[32] J. G. Lin, S. Q. Zang, Z. F. Tian, Y. Z. Li, Y. Y. Xu, H. Z. Zhu,

Q. J. Meng, CrystEngComm 2007, 9, 915.[33] Q. Y. Liu, D. Q. Yuan, L. Xu, Cryst. Growth Des. 2007, 7, 1832.[34] L. L. Wen, Z. D. Lu, X. M. Ren, C. Y. Duan, Q. J. Meng, S. Gao,

Cryst. Growth Des. 2009, 9, 227.[35] D. N. Dybtsev, H. Chun, K. Kim, Angew. Chem. Int. Ed. 2004,

43, 5033.[36] A. P. Côté, G. K. H. Shimizu, Chem. Eur. J. 2003, 9, 5361.[37] B. D. Chandler, G. D. Enright, S. Pawsey, J. A. Ripmeester, D. T.

Cramb, G. K. H. Shimizu, Nat. Mater. 2008, 7, 229.[38] D. J. Hoffart, S. A. Dalrymple, G. K. H. Shimizu, Inorg. Chem.

2005, 44, 8868.[39] B. D. Chandler, A. P. Cote, D. T. Cramb, J. M. Hill, G. K. H.

Shimizu, Chem. Commun. 2002, 1900.[40] S. K. Makinen, N. J. Melcer, M. Parvez, G. K. H. Shimizu,

Chem. Eur. J. 2001, 7, 5176.[41] S. A. Dalrymple, G. K. H. Shimizu, Chem. Eur. J. 2002, 8, 3010.[42] G. Wu, X. F. Wang, X. L. Guo, L. Yu, Z. Anorg. Allg. Chem.

2010, 636, 652.

Received: October 16, 2010Published Online: January 5, 2011

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Synthesis, Structure, and Physical Properties of a Barium Complex with 5-Sulfoisophthalic Acid Sodium Salt