Poly[tetra-μ2-l-lactato-indium(III)sodium(I)]

Wei, J.-J.; Zhang, N.; Wang, Y.-L.; Liu, Q.-Y.

doi:10.1107/S0108270111013606

metal-organic compounds

STRUCTURAL
CHEMISTRY

ISSN: 2053-2296

Volume 67| Part 5| May 2011| Pages m145-m148

doi:10.1107/S0108270111013606

Poly[tetra-μ₂-L-lactato-indium(III)sodium(I)]

Jia-Jia Wei,^a Na Zhang,^a Yu-Ling Wang ^a and Qing-Yan Liu ^a ^*

^aCollege of Chemistry and Chemical Engineering, Jiangxi Normal University, Nanchang, Jiangxi 330022, People's Republic of China
^*Correspondence e-mail: qyliuchem@hotmail.com

(Received 15 March 2011; accepted 11 April 2011; online 15 April 2011)

The asymmetric unit of the title compound, [InNa(C₃H₅O₃)₄]_n, consists of one In^III ion, one Na^I ion and four crystallographically independent L-lactate monoanions. The coordination of the In^III ion is composed of five carboxylate O and two hydroxy O atoms in a distorted pentagonal–bipyramidal coordination geometry. The Na^I ion is six-coordinated by four carboxylate O atoms and two hydroxy O atoms from four L-lactate ligands in a distorted octahedral geometry. Each In^III ion is coordinated by four surrounding L-lactate ligands to form an [In(L-lactate)₄]⁻ unit, which is further linked by Na^I ions through Na—O bonds to give a two-dimensional layered structure. Hydrogen bonds between the hydroxy groups and carboxylate O atoms are observed between neighbouring layers.

Comment

The construction of coordination polymers with desired properties from multifunctional ligands with metal ions is of current interest and great importance because these materials can exhibit a variety of physical properties, such as catalysis, molecular magnetism, photoluminescence, adsorption and phase separation (Janiak, 2003 ; Kitagawa et al., 2004 ; O'Keeffe et al., 2000 ). The rational synthesis of these materials, however, remains a great challenge. Ionothermal synthesis, a new synthetic methodology developed recently involving the use of an ionic liquid as both solvent and template in the preparation of crystalline solids, offers many advantages over traditional hydrothermal and solvothermal materials synthesis methods (Parnham & Morris, 2007 ; Reichert et al., 2006 ). Compared with traditional hydrothermal and solvothermal methods, the change from molecular to ionic reaction media leads to new types of materials being accessible, with structural properties that may be traced directly to the chemistry of the ionic liquid (IL) (Chen et al., 2008 ; Zhang et al., 2010 ). Therefore, the ionic species of ILs may control the structures of the materials formed in ionothermal synthesis. There are some examples in which ILs have been successfully applied to the syntheses of novel coordination compounds (Chen et al., 2009 ; Xu et al., 2007 ). Of particular interest is a recent study by Morris and co-workers (Lin et al., 2007 ) on the use of an enantiopure anion as one component of the IL to induce homochirality in a nickel(II) structure constructed of entirely achiral building blocks, despite the fact that the anion of the IL is not occluded by the material. Nevertheless, there are still relatively few examples of coordination polymers prepared by ionothermal reaction to date.

The In^III ion is liable to hydrolysis, which limits its use in the construction of coordination compounds under hydrothermal or solvothermal conditions. However, In^III ions can be used to construct new frameworks under ionothermal conditions because the In^III ion will not hydrolyse in IL solvents. A series of In compounds prepared under ionothermal reaction conditions has been reported recently (Zhang et al., 2008 ). We report here the title indium compound, poly[tetra-μ₂-L-lactato-indium(III)sodium(I)], (I). To the best of our knowledge, no indium compound based on the lactate ligand has been reported previously.

The asymmetric unit of (I) consists of one In^III ion, one Na^I ion and four L-lactate monoanions. As depicted in Fig. 1, the In1 ion is seven-coordinated by five carboxylate O atoms (O1, O4, O7, O8 and O10) and two hydroxy O atoms (O3 and O6) from four L-lactate ligands in a pentagonal–bipyramidal coordination environment, with atoms O6 and O10 occupying the apical positions. The In—O bond lengths range from 2.133 (2) to 2.356 (2) Å and the O—In—O bond angles vary from 55.29 (8) to 164.80 (9)° (Table 1). The Na1 ion is six-coordinated by two carboxylate O atoms [O2 and O5ⁱⁱ; symmetry code: (ii) x − 1, y, z] and two hydroxy O atoms [O12ⁱ and O9ⁱⁱⁱ; symmetry codes: (i) −x + 1, y + $[{1\over 2}]$ , −z + $[{1\over 2}]$ ; (iii) −x + 1, y − $[{1\over 2}]$ , −z + $[{1\over 2}]$ ] in a distorted square-planar geometry, with two carboxylate O atoms (O8ⁱⁱⁱ and O11ⁱ) in the apical positions. The Na1 ion is surrounded by four L-lactate ligands, with Na1—O distances varying from 2.364 (3) to 2.476 (3) Å (Fig. 1 and Table 1). The [NaO₆] octahedron is distorted, with O—Na—O bond angles varying from 65.13 (8) to 175.47 (11)° (Table 1).

Though all the L-lactate ligands bridge one In^III ion and one Na^I ion, the four crystallographically independent L-lactate ligands display three different coordination modes. The first type of L-lactate ligand chelates an In^III ion through its hydroxy O atom (O3) and one carboxylate O atom (O1), and bridges an Na^I ion through its second carboxylate O atom (O2) (Fig. 2). The second type of L-lactate ligand coordination is similar to the first; it chelates an Na^I ion through its hydroxy O atom (O12) and one carboxylate O atom (O11), and bridges an In^III ion through its second carboxylate O atom (O10). The third type of L-lactate ligand employs its carboxylate group (O7 and O8) to chelate an In^III ion, and its hydroxy O atom (O9) and one of its carboxylate O atoms (O8) to chelate an Na^I ion. Therefore, there is a μ₂-O (O8) bridge present in this type of L-lactate ligand.

Each In^III ion is coordinated by four surrounding L-lactate ligands to form an [In(L-lactate)₄]⁻ unit (Fig. 2). Each of these [In(L-lactate)₄]⁻ units is linked by four neighbouring Na^I ions through Na—O bonds to generate a two-dimensional layer along the ab plane (Fig. 3). Within the layer, there are hydrogen bonds between the hydroxy groups and the carboxylate O atoms [O3⋯O2ⁱ and O6⋯O5^iv; symmetry code: (iv) −x + 2, y + $[{1\over 2}]$ , −z + $[{1\over 2}]$ ] (Table 2). The two-dimensional layers are stacked along the c direction to produce the crystal packing (Fig. 4). Interlayer hydrogen bonds are observed between the hydroxy groups and the carboxylate O atoms [O9⋯O10^v and O12⋯O7^vi; symmetry codes: (v) x + $[{1\over 2}]$ , −y + $[{3\over 2}]$ , −z; (vi) x − $[{1\over 2}]$ , −y + $[{1\over 2}]$ , −z] (Table 2).

Some coordination compounds incorporating the lactate ligand have been reported previously. Most of them are mononuclear structures, such as [Co(lactate)₂(H₂O)₂]·H₂O (Carballo et al., 2002 ), [Mn(lactate)₂(H₂O)₂] (Lis, 1982 ) and [Al(lactate)₃] (Bombi et al., 1990 ). A few compounds with two-dimensional structures containing bridging lactate ligands have also been reported. However, all of them are homometallic compounds. For example, {[Eu(lactate)₂(H₂O)₂]ClO₄}_n possesses a cationic two-dimensional laminar layer charged with the perchlorate ions (Qu et al., 2008 ). In the [Cu(lactate)₂]_n complex (Balboa et al., 2007 ), the lactate ligand chelates a Cu^II ion through its hydroxy O atom and one carboxylate O atom, and bridges one Cu^II ion through the second carboxylate O atom, to generate a neutral two-dimensional framework where the basic structural unit is the mononuclear [Cu(lactate)₂] unit.

Figure 1
The structure of (I)

, showing the atom-numbering scheme. Displacement ellipsoids are drawn at the 30% probability level. Methyl H atoms have been omitted for clarity. [Symmetry codes: (i) −x + 1, y + $[{1\over 2}]$ , −z + $[{1\over 2}]$ ; (ii) x − 1, y, z; (iii) −x + 1, y − $[{1\over 2}]$ , −z + $[{1\over 2}]$ .]

Figure 2
A view of the [In(L-lactate)₄]⁻ unit surrounded by four Na^I ions. [Symmetry codes: (i) −x + 1, y + $[{1\over 2}]$ , −z + $[{1\over 2}]$ ; (iii) −x + 1, y − $[{1\over 2}]$ , −z + $[{1\over 2}]$ ; (vi) x + 1, y, z.]

Figure 3
A perspective view of the two-dimensional layered structure of (I)

. H atoms have been omitted for clarity. Dashed lines between hydroxy O and carboxylate O atoms indicate hydrogen bonds. [Symmetry codes: (i) −x + 1, y + $[{1\over 2}]$ , −z + $[{1\over 2}]$ ; (iv) −x + 2, y + $[{1\over 2}]$ , −z + $[{1\over 2}]$ .]

Figure 4
A view of the packing of (I)

along the a axis. H atoms have been omitted for clarity. Dashed lines between hydroxy O and carboxylate O atoms indicate interlayer hydrogen bonds.

Experimental

In(NO₃)₃·4.5H₂O (229.2 mg, 0.6 mmol) and the monosodium salt of 5-sulfoisophthalic acid (53.6 mg, 0.2 mmol) were mixed with 1-ethyl-3-methylimidazolium L-lactate (0.6 g) in a 25 ml Parr Teflon-lined stainless steel vessel. The vessel was sealed and heated to 413 K. The temperature was maintained for 12 d and then the mixture was allowed to cool naturally to obtain colourless crystals of (I) [yield 51%, based on In(NO₃)₃·4.5H₂O]. IR (KBr pellet, ν, cm⁻¹): 3465, 3391, 3105, 2950, 1638, 1598, 1564, 1473, 1417, 1254, 1124, 1073, 954, 868, 776, 666, 588, 540, 518.

Crystal data

[InNa(C₃H₅O₃)₄]
M_r = 494.09
Orthorhombic, P 2₁ 2₁ 2₁
a = 9.4744 (12) Å
b = 9.5803 (12) Å
c = 19.145 (2) Å
V = 1737.7 (4) Å³
Z = 4
Mo Kα radiation
μ = 1.45 mm⁻¹
T = 296 K
0.18 × 0.13 × 0.09 mm

Data collection

Bruker APEXII area-detector diffractometer
Absorption correction: multi-scan (SADABS; Sheldrick, 1996 ) T_min = 0.781, T_max = 0.881
10916 measured reflections
4259 independent reflections
3680 reflections with I > 2σ(I)
R_int = 0.029

Refinement

R[F² > 2σ(F²)] = 0.029
wR(F²) = 0.057
S = 1.02
4259 reflections
247 parameters
H atoms treated by a mixture of independent and constrained refinement
Δρ_max = 0.45 e Å⁻³
Δρ_min = −0.42 e Å⁻³
Absolute structure: Flack (1983 ), with 1766 Friedel pairs
Flack parameter: 0.03 (2)

Table 1
Selected geometric parameters (Å, °)

In1—O10	2.133 (2)
In1—O4	2.162 (2)
In1—O1	2.183 (2)
In1—O6	2.217 (2)
In1—O3	2.255 (2)
In1—O8	2.338 (2)
In1—O7	2.356 (2)
Na1—O12ⁱ	2.364 (3)
Na1—O5ⁱⁱ	2.423 (3)
Na1—O2	2.435 (3)
Na1—O8ⁱⁱⁱ	2.437 (2)
Na1—O11ⁱ	2.462 (2)
Na1—O9ⁱⁱⁱ	2.476 (3)

O10—In1—O4	122.10 (9)
O10—In1—O1	91.88 (9)
O4—In1—O1	81.77 (10)
O10—In1—O6	164.80 (9)
O4—In1—O6	73.05 (8)
O1—In1—O6	91.77 (10)
O10—In1—O3	83.36 (9)
O1—In1—O3	72.36 (9)
O6—In1—O3	83.70 (9)
O10—In1—O8	93.10 (8)
O6—In1—O8	75.68 (8)
O3—In1—O8	74.12 (8)
O10—In1—O7	87.13 (9)
O4—In1—O7	81.37 (9)
O6—In1—O7	94.55 (9)
O8—In1—O7	55.29 (8)
O12ⁱ—Na1—O2	99.82 (12)
O5ⁱⁱ—Na1—O2	88.19 (8)
O12ⁱ—Na1—O8ⁱⁱⁱ	110.79 (10)
O5ⁱⁱ—Na1—O8ⁱⁱⁱ	77.75 (9)
O2—Na1—O8ⁱⁱⁱ	85.24 (10)
O12ⁱ—Na1—O11ⁱ	66.95 (9)
O5ⁱⁱ—Na1—O11ⁱ	103.98 (11)
O2—Na1—O11ⁱ	98.95 (12)
O8ⁱⁱⁱ—Na1—O11ⁱ	175.47 (11)
O12ⁱ—Na1—O9ⁱⁱⁱ	84.43 (10)
O5ⁱⁱ—Na1—O9ⁱⁱⁱ	92.82 (11)
O8ⁱⁱⁱ—Na1—O9ⁱⁱⁱ	65.13 (8)
O11ⁱ—Na1—O9ⁱⁱⁱ	110.47 (11)
Symmetry codes: (i) $[-x+1, y+{\script{1\over 2}}, -z+{\script{1\over 2}}]$ ; (ii) x-1, y, z; (iii) $[-x+1, y-{\script{1\over 2}}, -z+{\script{1\over 2}}]$ .

Table 2
Hydrogen-bond geometry (Å, °)

D—H⋯A	D—H	H⋯A	D⋯A	D—H⋯A
O3—H3⋯O2ⁱ	0.86 (4)	1.76 (4)	2.620 (3)	177 (4)
O6—H6⋯O5^iv	0.82 (4)	1.77 (4)	2.578 (4)	170 (4)
O9—H9⋯O10^v	0.83 (4)	2.26 (4)	3.087 (4)	173 (4)
O12—H12⋯O7^vi	0.87 (4)	2.05 (4)	2.916 (3)	173 (4)
Symmetry codes: (i) $[-x+1, y+{\script{1\over 2}}, -z+{\script{1\over 2}}]$ ; (iv) $[-x+2, y+{\script{1\over 2}}, -z+{\script{1\over 2}}]$ ; (v) $[x+{\script{1\over 2}}]$ , $[-y+{\script{3\over 2}}, -z]$ ; (vi) $[x-{\script{1\over 2}}, -y+{\script{1\over 2}}, -z]$ .

H atoms bonded to C atoms were placed in calculated positions and treated using a riding-model approximation, with C—H = 0.96 Å and U_iso(H) = 1.5U_eq(C) for methyl groups, and C—H = 0.98 Å and U_iso(H) = 1.2U_eq(C) for methylidyne groups. Hydroxy H atoms were located in a difference map and refined with U_iso(H) = 1.5U_eq(O).

Data collection: APEX2 (Bruker, 2008 ); cell refinement: SAINT (Bruker, 2008); data reduction: SAINT; program(s) used to solve structure: SHELXS97 (Sheldrick, 2008 ); program(s) used to refine structure: SHELXL97 (Sheldrick, 2008); molecular graphics: SHELXTL (Sheldrick, 2008) and DIAMOND (Brandenburg, 2005 ); software used to prepare material for publication: SHELXTL.

Supporting information

Crystal structure: contains datablocks I, global. DOI: 10.1107/S0108270111013606/lg3055sup1.cif

Structure factors: contains datablock I. DOI: 10.1107/S0108270111013606/lg3055Isup2.hkl

Comment top

The construction of coordination polymers with desired properties from multifunctional ligands with metal ions is of current interest and great importance because these materials can exhibit a variety of physical properties, such as catalysis, molecular magnetism, photoluminescence, adsorption and phase separation (Janiak, 2003; Kitagawa et al., 2004; O'Keeffe et al., 2000). The rational synthesis of these materials, however, remains a great challenge. Ionothermal synthesis, a new synthetic methodology developed recently involving the use of an ionic liquid as solvent and template in the preparation of crystalline solids, offers many advantages over traditional hydrothermal and solvothermal materials synthesis methods (Parnham & Morris, 2007; Reichert et al., 2006). Compared with traditional hydrothermal and solvothermal methods, the change from molecular to ionic reaction media leads to new types of materials being accessible, with structural properties that may be traced directly to the chemistry of the ionic liquid (IL) (Chen et al., 2008; Zhang et al., 2010). Therefore, the ionic species of ILs may control the structures of the materials formed in ionothermal synthesis. There are some examples in which ILs have been successfully applied to the syntheses of novel coordination compounds (Chen et al., 2009; Xu et al., 2007). Of particular interest is a recent study by Morris and co-workers (Lin et al., 2007) on the use of an enantiopure anion as one component of the IL to induce homochirality in a nickel(II) structure constructed of entirely achiral building blocks, despite the fact that the anion of the IL is not occluded by the material. Nevertheless, there are still relatively few examples of coordination polymers prepared under ionothermal reaction to date.

The In^III ion is liable to hydrolysis, which limits its use in the construction of coordination compounds under hydrothermal or solvothermal conditions. However, In^III ions can be used to construct new frameworks under ionothermal conditions beacuse the In^III ion will not hydrolyse in IL solvents. A series of In compounds prepared under ionothermal reaction conditions have been reported recently (Zhang et al., 2008). We report here the title indium compound, [InNa(C₃H₅O₃)₄]_n, (I). To the best of our knowledge, no indium compound based on the lactate ligand has been reported previously.

The asymmetric unit of (I) consists of one In^III ion, one Na^I ion and four L-lactate monoanions. As depicted in Fig. 1, the In1 ion is seven-coordinated by five carboxylate O atoms (O1, O4, O7, O8 and O10) and two hydroxy O atoms (O3 and O6) from four L-lactate ligands in a pentagonal–bipyramidal coordination environment, with atoms O6 and O10 occupying the apical positions. The In—O bond lengths range from 2.133 (2) to 2.356 (2) Å and the O—In—O bond angles vary from 55.29 (8) to 164.80 (9)° (Table 1). The Na1 ion is six-coordinated by two carboxylate O atoms [O2 and O5ⁱⁱ; symmetry code: (ii) x - 1, y, z] and two hydroxy O atoms [O12ⁱ and O9ⁱⁱⁱ; symmetry codes: (i) -x + 1, y + 1/2, -z + 1/2; (iii) -x + 1, y - 1/2, -z + 1/2] in a distorted square-planar geometry, with two carboxylate O atoms (O8ⁱⁱⁱ and O11ⁱ) in the apical positions. The Na1 ion is surrounded by four L-lactate ligands, with Na1—O distances varying from 2.364 (3) to 2.476 (3) Å (Fig. 1 and Table 1). The [NaO₆] octahedron is distorted, with O—Na—O bond angles varying from 65.13 (8) to 175.47 (11)° (Table 1).

Though all the L-lactate ligands bridge one In^III ion and one Na^I ion, the four crystallographically independent L-lactate ligands display three different coordination modes. The first type of L-lactate ligand chelates an In^III ion through its hydroxy O atom (O3) and one carboxylate O atom (O1), and bridges an Na^I ion through its second carboxylate O atom (O2) (Fig. 2). The second type of L-lactate ligand coordination is similar to the first: it chelates an Na^I ion through its hydroxy O atom (O12) and one carboxylate O atom (O11), and bridges an In^III ion through its second carboxylate O atom (O10). The third type of L-lactate ligand employs its carboxylate group (O7 and O8) to chelate an In^III ion, and its hydroxy O atom (O9) and one of its carboxylate O atoms (O8) to chelate an Na^I ion. Therefore, there is a µ₂-O (O8) bridge present in this type of L-lactate ligand.

Each In^III ion is coordinated by four surrounding L-lactate ligands to form an [In(L-lactate)₄]^- unit (Fig. 2). Each of these [In(L-lactate)₄]^- units is linked by four neighbouring Na^I ions through Na—O bonds to generate a two-dimensional layer along the ab plane (Fig. 3). Within the layer, there are hydrogen bonds between the hydroxy groups and the carboxylate O atoms [O3···O2ⁱ and O6···O5^iv; symmetry code: (iv) -x + 2, y + 1/2, -z + 1/2] (Table 2). The two-dimensional layers are stacked along the c direction to produce the crystal packing (Fig. 4). Interlayer hydrogen bonds are observed between the hydroxy groups and the carboxylate O atoms [O9···O10^v and O12···O7^vi; symmetry codes: (v) x + 1/2, -y + 3/2, -z; (vi) x - 1/2, -y + 1/2, -z.] (Table 2).

Some coordination compounds with the lactate ligand have been reported previously. Most of them are mononuclear structures, such as [Co(lactate)₂(H₂O)₂](H₂O) (Carballo et al., 2002), [Mn(lactate)₂(H₂O)₂] (Lis, 1982) and [Al(lactate)₃] (Bombi et al., 1990). A few compounds with two-dimensional structures containing bridging lactate ligands have also been reported. However, all of them are homometallic compounds. For example, the {[Eu(lactate)₂(H₂O)₂](ClO₄)}_n compound possess a cationic two-dimensional laminar layer charged with the perchlorate ions (Qu et al., 2008). In the [Cu(lactate)₂]_n complex (Balboa et al., 2007), the lactate ligand chelates a Cu^II ion through its hydroxy O atom and one carboxylate O atom, and bridges one Cu^II ion through the second carboxylate O atom, to generate a neutral two-dimensional framework where the basic structrual unit is the mononuclear [Cu(lactate)₂] unit.

Related literature top

For related literature, see: Balboa et al. (2007); Bombi et al. (1990); Carballo et al. (2002); Chen et al. (2008, 2009); Janiak (2003); Kitagawa et al. (2004); Lin et al. (2007); Lis (1982); O'Keeffe et al. (2000); Parnham & Morris (2007); Qu et al. (2008); Reichert et al. (2006); Xu et al. (2007); Zhang et al. (2008, 2010).

Experimental top

In(NO₃)₃.4.5H₂O (229.2 mg, 0.6 mmol) and 5-sulfoisophthalic acid monosodium salt (53.6 mg, 0.2 mmol) were mixed with 0.6 g 1-ethyl-3-methylimidazolium-L-lactate in a Parr 25 ml Teflon-lined stainless steel vessel. The vessel was sealed and heated to 413 K. The temperature was maintained for 12 d and then the mixture was cooled naturally to obtain colourless crystals of (I) [yield 51%, based on In(NO₃)₃.4.5H₂O]. Spectroscopic analysis: IR (KBr pellet, ν, cm^-1): 3465, 3391, 3105, 2950, 1638, 1598, 1564, 1473, 1417, 1254, 1124, 1073, 954, 868, 776, 666, 588, 540, 518.

Computing details top

Data collection: APEX2 (Bruker, 2008); cell refinement: SAINT (Bruker, 2008); data reduction: SAINT (Bruker, 2008); program(s) used to solve structure: SHELXS97 (Sheldrick, 2008); program(s) used to refine structure: SHELXL97 (Sheldrick, 2008); molecular graphics: SHELXTL (Sheldrick, 2008) and DIAMOND (Brandenburg, 2005); software used to prepare material for publication: SHELXTL (Sheldrick, 2008).

Figures top

	Fig. 1. The structure of (I), showing the atom-numbering scheme. Displacement ellipsoids are drawn at the 30% probability level. Methyl H atoms have been omitted for clarity. [Symmetry codes: (i) -x + 1, y + 1/2, -z + 1/2; (ii) x - 1, y, z; (iii) -x + 1, y - 1/2, -z + 1/2.]
	Fig. 2. A view of the [In(L-lactate)₄]^- unit surrounded by four Na^I ions. [Symmetry codes: (i) -x + 1, y + 1/2, -z + 1/2; (iii) -x + 1, y - 1/2, -z + 1/2; (vi) x + 1, y, z.]
	Fig. 3. A perspective view of the two-dimensional layered structure of (I). H atoms have been omitted for clarity. Dotted lines between hydroxy O and carboxylate O atoms indicate hydrogen bonds. [Symmetry codes: (i) -x + 1, y + 1/2, -z + 1/2; (iv) -x + 2, y + 1/2, -z + 1/2.]
	Fig. 4. A view of the packing of (I), along the a axis. H atoms have been omitted for clarity. Dotted lines between hydroxy O and carboxylate O atoms indicate interlayer hydrogen bonds.

Poly[tetra-µ₂-L-lactato-indium(III)sodium(I)] top

Crystal data top

[InNa(C₃H₅O₃)₄]	D_x = 1.889 Mg m⁻³
M_r = 494.09	Mo Kα radiation, λ = 0.71073 Å
Orthorhombic, P2₁2₁2₁	Cell parameters from 4051 reflections
a = 9.4744 (12) Å	θ = 2.4–27.8°
b = 9.5803 (12) Å	µ = 1.45 mm⁻¹
c = 19.145 (2) Å	T = 296 K
V = 1737.7 (4) Å³	Prism, colourless
Z = 4	0.18 × 0.13 × 0.09 mm
F(000) = 992

Data collection top

Bruker APEXII area-detector diffractometer	4259 independent reflections
Radiation source: fine-focus sealed tube	3680 reflections with I > 2σ(I)
Graphite monochromator	R_int = 0.029
ω scans	θ_max = 29.1°, θ_min = 2.1°
Absorption correction: multi-scan (SADABS; Sheldrick, 1996)	h = −10→12
T_min = 0.781, T_max = 0.881	k = −12→11
10916 measured reflections	l = −25→24

Refinement top

Refinement on F²	Secondary atom site location: difference Fourier map
Least-squares matrix: full	Hydrogen site location: inferred from neighbouring sites
R[F² > 2σ(F²)] = 0.029	H atoms treated by a mixture of independent and constrained refinement
wR(F²) = 0.057	w = 1/[σ²(F_o²) + (0.0226P)² + 0.1617P] where P = (F_o² + 2F_c²)/3
S = 1.02	(Δ/σ)_max = 0.001
4259 reflections	Δρ_max = 0.45 e Å⁻³
247 parameters	Δρ_min = −0.42 e Å⁻³
0 restraints	Absolute structure: Flack (1983), with 1766 Friedel pairs
Primary atom site location: structure-invariant direct methods	Absolute structure parameter: 0.03 (2)

Crystal data top

[InNa(C₃H₅O₃)₄]	V = 1737.7 (4) Å³
M_r = 494.09	Z = 4
Orthorhombic, P2₁2₁2₁	Mo Kα radiation
a = 9.4744 (12) Å	µ = 1.45 mm⁻¹
b = 9.5803 (12) Å	T = 296 K
c = 19.145 (2) Å	0.18 × 0.13 × 0.09 mm

Data collection top

Bruker APEXII area-detector diffractometer	4259 independent reflections
Absorption correction: multi-scan (SADABS; Sheldrick, 1996)	3680 reflections with I > 2σ(I)
T_min = 0.781, T_max = 0.881	R_int = 0.029
10916 measured reflections

Refinement top

R[F² > 2σ(F²)] = 0.029	H atoms treated by a mixture of independent and constrained refinement
wR(F²) = 0.057	Δρ_max = 0.45 e Å⁻³
S = 1.02	Δρ_min = −0.42 e Å⁻³
4259 reflections	Absolute structure: Flack (1983), with 1766 Friedel pairs
247 parameters	Absolute structure parameter: 0.03 (2)
0 restraints

Special details top

Geometry. All e.s.d.'s (except the e.s.d. in the dihedral angle between two l.s. planes) are estimated using the full covariance matrix. The cell e.s.d.'s are taken into account individually in the estimation of e.s.d.'s in distances, angles and torsion angles; correlations between e.s.d.'s in cell parameters are only used when they are defined by crystal symmetry. An approximate (isotropic) treatment of cell e.s.d.'s is used for estimating e.s.d.'s involving l.s. planes.

Refinement. Refinement of F² against ALL reflections. The weighted R-factor wR and goodness of fit S are based on F², conventional R-factors R are based on F, with F set to zero for negative F². The threshold expression of F² > σ(F²) is used only for calculating R-factors(gt) etc. and is not relevant to the choice of reflections for refinement. R-factors based on F² are statistically about twice as large as those based on F, and R-factors based on ALL data will be even larger.

Fractional atomic coordinates and isotropic or equivalent isotropic displacement parameters (Å²) top

	x	y	z	U_iso*/U_eq
In1	0.74771 (3)	0.528992 (19)	0.160204 (9)	0.02032 (6)
Na1	0.2434 (2)	0.48419 (11)	0.39058 (6)	0.0296 (3)
C1	0.5051 (4)	0.4774 (5)	0.2605 (2)	0.0243 (9)
C2	0.4461 (4)	0.6048 (4)	0.22333 (18)	0.0318 (9)
H2	0.4251	0.6776	0.2578	0.038*
C3	0.3134 (5)	0.5677 (6)	0.1845 (3)	0.085 (2)
H3A	0.2771	0.6493	0.1616	0.127*
H3B	0.2444	0.5329	0.2168	0.127*
H3C	0.3340	0.4973	0.1503	0.127*
C4	0.9811 (4)	0.4819 (5)	0.26467 (19)	0.0216 (9)
C5	0.9469 (4)	0.6319 (3)	0.28158 (16)	0.0243 (7)
H5	1.0317	0.6886	0.2742	0.029*
C6	0.9000 (5)	0.6482 (5)	0.35579 (17)	0.0564 (14)
H6A	0.8789	0.7446	0.3648	0.085*
H6B	0.9739	0.6178	0.3865	0.085*
H6C	0.8170	0.5928	0.3636	0.085*
C7	0.8894 (4)	0.6863 (3)	0.06632 (17)	0.0253 (7)
C8	0.9838 (4)	0.7789 (4)	0.02157 (17)	0.0265 (8)
H8	0.9957	0.7364	−0.0246	0.032*
C9	1.1264 (4)	0.7923 (4)	0.05664 (19)	0.0367 (9)
H9A	1.1866	0.8505	0.0288	0.055*
H9B	1.1682	0.7015	0.0614	0.055*
H9C	1.1147	0.8334	0.1020	0.055*
C10	0.6526 (4)	0.2970 (3)	0.07842 (16)	0.0248 (7)
C11	0.5578 (4)	0.2150 (3)	0.02921 (17)	0.0261 (8)
H11	0.5508	0.2644	−0.0155	0.031*
C12	0.4134 (4)	0.2011 (5)	0.0607 (2)	0.0495 (11)
H12A	0.3534	0.1503	0.0294	0.074*
H12B	0.3745	0.2923	0.0687	0.074*
H12C	0.4200	0.1520	0.1043	0.074*
O1	0.6229 (3)	0.4288 (3)	0.24191 (13)	0.0291 (6)
O2	0.4306 (3)	0.4265 (3)	0.30834 (13)	0.0333 (7)
O3	0.5494 (3)	0.6559 (2)	0.17475 (12)	0.0272 (6)
H3	0.553 (4)	0.745 (4)	0.1792 (18)	0.041*
O4	0.9176 (3)	0.4232 (2)	0.21391 (12)	0.0271 (6)
O5	1.0742 (3)	0.4246 (3)	0.30051 (13)	0.0287 (7)
O6	0.8383 (3)	0.6802 (2)	0.23555 (12)	0.0271 (6)
H6	0.856 (4)	0.760 (4)	0.2242 (19)	0.041*
O7	0.9266 (3)	0.5612 (2)	0.07629 (12)	0.0342 (6)
O8	0.7802 (2)	0.7326 (2)	0.09477 (11)	0.0265 (6)
O9	0.9175 (3)	0.9112 (3)	0.01432 (14)	0.0357 (6)
H9	0.971 (5)	0.961 (5)	−0.009 (2)	0.054*
O10	0.6278 (3)	0.4302 (2)	0.07989 (12)	0.0312 (6)
O11	0.7416 (4)	0.2405 (2)	0.11515 (11)	0.0389 (6)
O12	0.6205 (3)	0.0815 (3)	0.01805 (14)	0.0397 (7)
H12	0.566 (5)	0.043 (5)	−0.013 (2)	0.060*

Atomic displacement parameters (Å²) top

	U¹¹	U²²	U³³	U¹²	U¹³	U²³
In1	0.02124 (10)	0.01809 (9)	0.02163 (9)	0.00056 (17)	−0.00087 (17)	0.00144 (8)
Na1	0.0299 (7)	0.0282 (6)	0.0307 (6)	−0.0021 (10)	−0.0040 (9)	−0.0015 (5)
C1	0.034 (2)	0.0155 (18)	0.023 (2)	−0.0036 (19)	0.0004 (17)	−0.0001 (19)
C2	0.033 (2)	0.0273 (19)	0.036 (2)	0.0079 (16)	0.0159 (17)	0.0079 (15)
C3	0.024 (2)	0.137 (5)	0.093 (4)	−0.008 (3)	−0.003 (2)	0.070 (4)
C4	0.0196 (19)	0.019 (2)	0.027 (2)	−0.0005 (17)	0.0023 (16)	0.0000 (19)
C5	0.0239 (19)	0.0198 (16)	0.0291 (18)	0.0022 (14)	−0.0063 (14)	0.0004 (14)
C6	0.080 (4)	0.060 (3)	0.029 (2)	0.038 (3)	−0.006 (2)	−0.0077 (19)
C7	0.032 (2)	0.0237 (17)	0.0203 (16)	−0.0028 (14)	0.0023 (15)	−0.0037 (14)
C8	0.033 (2)	0.0228 (18)	0.0237 (17)	0.0046 (14)	0.0049 (16)	−0.0011 (14)
C9	0.034 (2)	0.039 (2)	0.037 (2)	−0.0011 (18)	0.0059 (18)	0.0003 (17)
C10	0.0251 (19)	0.0284 (18)	0.0209 (16)	−0.0058 (15)	0.0015 (14)	−0.0040 (14)
C11	0.035 (2)	0.0156 (16)	0.0275 (17)	0.0014 (14)	−0.0070 (15)	−0.0021 (13)
C12	0.034 (3)	0.052 (3)	0.062 (3)	−0.009 (2)	−0.006 (2)	−0.013 (2)
O1	0.0270 (15)	0.0249 (14)	0.0354 (14)	0.0068 (11)	0.0075 (12)	0.0107 (12)
O2	0.0410 (18)	0.0241 (15)	0.0349 (16)	0.0030 (14)	0.0168 (14)	0.0095 (13)
O3	0.0323 (14)	0.0143 (11)	0.0348 (14)	−0.0010 (10)	0.0106 (11)	0.0048 (10)
O4	0.0303 (15)	0.0183 (12)	0.0327 (14)	0.0050 (11)	−0.0054 (11)	−0.0058 (11)
O5	0.0281 (16)	0.0233 (14)	0.0347 (15)	0.0043 (13)	−0.0076 (13)	−0.0022 (12)
O6	0.0347 (15)	0.0134 (12)	0.0331 (13)	0.0007 (11)	−0.0124 (11)	0.0033 (10)
O7	0.0445 (17)	0.0195 (13)	0.0385 (14)	0.0033 (11)	0.0089 (12)	0.0018 (11)
O8	0.0252 (18)	0.0300 (12)	0.0244 (10)	−0.0013 (10)	0.0047 (10)	−0.0023 (9)
O9	0.0386 (16)	0.0256 (13)	0.0429 (15)	0.0057 (12)	0.0088 (13)	0.0109 (12)
O10	0.0431 (16)	0.0186 (12)	0.0320 (13)	−0.0054 (11)	−0.0009 (12)	−0.0040 (10)
O11	0.0370 (15)	0.0399 (13)	0.0397 (12)	−0.0017 (19)	−0.0129 (19)	−0.0079 (10)
O12	0.0471 (18)	0.0239 (13)	0.0481 (16)	0.0074 (12)	−0.0173 (14)	−0.0151 (12)

Geometric parameters (Å, º) top

In1—O10	2.133 (2)	C6—H6B	0.9600
In1—O4	2.162 (2)	C6—H6C	0.9600
In1—O1	2.183 (2)	C7—O8	1.250 (4)
In1—O6	2.217 (2)	C7—O7	1.264 (4)
In1—O3	2.255 (2)	C7—C8	1.523 (5)
In1—O8	2.338 (2)	C8—O9	1.422 (4)
In1—O7	2.356 (2)	C8—C9	1.514 (5)
Na1—O12ⁱ	2.364 (3)	C8—H8	0.9800
Na1—O5ⁱⁱ	2.423 (3)	C9—H9A	0.9600
Na1—O2	2.435 (3)	C9—H9B	0.9600
Na1—O8ⁱⁱⁱ	2.437 (2)	C9—H9C	0.9600
Na1—O11ⁱ	2.462 (2)	C10—O11	1.224 (4)
Na1—O9ⁱⁱⁱ	2.476 (3)	C10—O10	1.298 (4)
C1—O2	1.254 (4)	C10—C11	1.521 (5)
C1—O1	1.261 (4)	C11—O12	1.426 (4)
C1—C2	1.520 (5)	C11—C12	1.501 (5)
C2—O3	1.436 (4)	C11—H11	0.9800
C2—C3	1.503 (6)	C12—H12A	0.9600
C2—H2	0.9800	C12—H12B	0.9600
C3—H3A	0.9600	C12—H12C	0.9600
C3—H3B	0.9600	O3—H3	0.86 (4)
C3—H3C	0.9600	O5—Na1^iv	2.423 (3)
C4—O5	1.245 (4)	O6—H6	0.82 (4)
C4—O4	1.273 (4)	O8—Na1ⁱ	2.437 (2)
C4—C5	1.509 (6)	O9—Na1ⁱ	2.476 (3)
C5—O6	1.431 (4)	O9—H9	0.83 (4)
C5—C6	1.497 (4)	O11—Na1ⁱⁱⁱ	2.462 (2)
C5—H5	0.9800	O12—Na1ⁱⁱⁱ	2.364 (3)
C6—H6A	0.9600	O12—H12	0.87 (4)

O10—In1—O4	122.10 (9)	C4—C5—H5	108.8
O10—In1—O1	91.88 (9)	C5—C6—H6A	109.5
O4—In1—O1	81.77 (10)	C5—C6—H6B	109.5
O10—In1—O6	164.80 (9)	H6A—C6—H6B	109.5
O4—In1—O6	73.05 (8)	C5—C6—H6C	109.5
O1—In1—O6	91.77 (10)	H6A—C6—H6C	109.5
O10—In1—O3	83.36 (9)	H6B—C6—H6C	109.5
O4—In1—O3	144.51 (8)	O8—C7—O7	120.1 (3)
O1—In1—O3	72.36 (9)	O8—C7—C8	121.6 (3)
O6—In1—O3	83.70 (9)	O7—C7—C8	118.3 (3)
O10—In1—O8	93.10 (8)	O9—C8—C9	111.2 (3)
O4—In1—O8	123.19 (9)	O9—C8—C7	108.4 (3)
O1—In1—O8	145.26 (8)	C9—C8—C7	108.9 (3)
O6—In1—O8	75.68 (8)	O9—C8—H8	109.5
O3—In1—O8	74.12 (8)	C9—C8—H8	109.5
O10—In1—O7	87.13 (9)	C7—C8—H8	109.5
O4—In1—O7	81.37 (9)	C8—C9—H9A	109.5
O1—In1—O7	159.40 (9)	C8—C9—H9B	109.5
O6—In1—O7	94.55 (9)	H9A—C9—H9B	109.5
O3—In1—O7	127.81 (8)	C8—C9—H9C	109.5
O8—In1—O7	55.29 (8)	H9A—C9—H9C	109.5
O12ⁱ—Na1—O5ⁱⁱ	168.59 (12)	H9B—C9—H9C	109.5
O12ⁱ—Na1—O2	99.82 (12)	O11—C10—O10	123.2 (3)
O5ⁱⁱ—Na1—O2	88.19 (8)	O11—C10—C11	122.3 (3)
O12ⁱ—Na1—O8ⁱⁱⁱ	110.79 (10)	O10—C10—C11	114.5 (3)
O5ⁱⁱ—Na1—O8ⁱⁱⁱ	77.75 (9)	O12—C11—C12	111.1 (3)
O2—Na1—O8ⁱⁱⁱ	85.24 (10)	O12—C11—C10	108.1 (3)
O12ⁱ—Na1—O11ⁱ	66.95 (9)	C12—C11—C10	109.6 (3)
O5ⁱⁱ—Na1—O11ⁱ	103.98 (11)	O12—C11—H11	109.3
O2—Na1—O11ⁱ	98.95 (12)	C12—C11—H11	109.3
O8ⁱⁱⁱ—Na1—O11ⁱ	175.47 (11)	C10—C11—H11	109.3
O12ⁱ—Na1—O9ⁱⁱⁱ	84.43 (10)	C11—C12—H12A	109.5
O5ⁱⁱ—Na1—O9ⁱⁱⁱ	92.82 (11)	C11—C12—H12B	109.5
O2—Na1—O9ⁱⁱⁱ	149.32 (10)	H12A—C12—H12B	109.5
O8ⁱⁱⁱ—Na1—O9ⁱⁱⁱ	65.13 (8)	C11—C12—H12C	109.5
O11ⁱ—Na1—O9ⁱⁱⁱ	110.47 (11)	H12A—C12—H12C	109.5
O2—C1—O1	124.1 (4)	H12B—C12—H12C	109.5
O2—C1—C2	116.6 (4)	C1—O1—In1	121.3 (3)
O1—C1—C2	119.3 (3)	C1—O2—Na1	142.5 (3)
O3—C2—C3	109.3 (3)	C2—O3—In1	117.67 (19)
O3—C2—C1	109.1 (3)	C2—O3—H3	108 (3)
C3—C2—C1	110.4 (4)	In1—O3—H3	121 (3)
O3—C2—H2	109.3	C4—O4—In1	120.5 (3)
C3—C2—H2	109.3	C4—O5—Na1^iv	139.2 (3)
C1—C2—H2	109.3	C5—O6—In1	117.89 (18)
C2—C3—H3A	109.5	C5—O6—H6	109 (3)
C2—C3—H3B	109.5	In1—O6—H6	121 (3)
H3A—C3—H3B	109.5	C7—O7—In1	91.5 (2)
C2—C3—H3C	109.5	C7—O8—In1	92.69 (19)
H3A—C3—H3C	109.5	C7—O8—Na1ⁱ	118.5 (2)
H3B—C3—H3C	109.5	In1—O8—Na1ⁱ	138.69 (10)
O5—C4—O4	124.1 (4)	C8—O9—Na1ⁱ	116.9 (2)
O5—C4—C5	117.0 (4)	C8—O9—H9	107 (3)
O4—C4—C5	118.9 (3)	Na1ⁱ—O9—H9	128 (3)
O6—C5—C6	109.7 (3)	C10—O10—In1	110.8 (2)
O6—C5—C4	109.3 (3)	C10—O11—Na1ⁱⁱⁱ	117.1 (2)
C6—C5—C4	111.5 (3)	C11—O12—Na1ⁱⁱⁱ	118.0 (2)
O6—C5—H5	108.8	C11—O12—H12	104 (3)
C6—C5—H5	108.8	Na1ⁱⁱⁱ—O12—H12	131 (3)

Symmetry codes: (i) −x+1, y+1/2, −z+1/2; (ii) x−1, y, z; (iii) −x+1, y−1/2, −z+1/2; (iv) x+1, y, z.

Hydrogen-bond geometry (Å, º) top

D—H···A	D—H	H···A	D···A	D—H···A
O3—H3···O2ⁱ	0.86 (4)	1.76 (4)	2.620 (3)	177 (4)
O6—H6···O5^v	0.82 (4)	1.77 (4)	2.578 (4)	170 (4)
O9—H9···O10^vi	0.83 (4)	2.26 (4)	3.087 (4)	173 (4)
O12—H12···O7^vii	0.87 (4)	2.05 (4)	2.916 (3)	173 (4)

Symmetry codes: (i) −x+1, y+1/2, −z+1/2; (v) −x+2, y+1/2, −z+1/2; (vi) x+1/2, −y+3/2, −z; (vii) x−1/2, −y+1/2, −z.

Experimental details

Crystal data
Chemical formula	[InNa(C₃H₅O₃)₄]
M_r	494.09
Crystal system, space group	Orthorhombic, P2₁2₁2₁
Temperature (K)	296
a, b, c (Å)	9.4744 (12), 9.5803 (12), 19.145 (2)
V (Å³)	1737.7 (4)
Z	4
Radiation type	Mo Kα
µ (mm⁻¹)	1.45
Crystal size (mm)	0.18 × 0.13 × 0.09

Data collection
Diffractometer	Bruker APEXII area-detector diffractometer
Absorption correction	Multi-scan (SADABS; Sheldrick, 1996)
T_min, T_max	0.781, 0.881
No. of measured, independent and observed [I > 2σ(I)] reflections	10916, 4259, 3680
R_int	0.029
(sin θ/λ)_max (Å⁻¹)	0.683

Refinement
R[F² > 2σ(F²)], wR(F²), S	0.029, 0.057, 1.02
No. of reflections	4259
No. of parameters	247
H-atom treatment	H atoms treated by a mixture of independent and constrained refinement
Δρ_max, Δρ_min (e Å⁻³)	0.45, −0.42
Absolute structure	Flack (1983), with 1766 Friedel pairs
Absolute structure parameter	0.03 (2)

Computer programs: APEX2 (Bruker, 2008), SAINT (Bruker, 2008), SHELXS97 (Sheldrick, 2008), SHELXL97 (Sheldrick, 2008), SHELXTL (Sheldrick, 2008) and DIAMOND (Brandenburg, 2005), SHELXTL (Sheldrick, 2008).

Selected geometric parameters (Å, º) top

In1—O10	2.133 (2)	Na1—O12ⁱ	2.364 (3)
In1—O4	2.162 (2)	Na1—O5ⁱⁱ	2.423 (3)
In1—O1	2.183 (2)	Na1—O2	2.435 (3)
In1—O6	2.217 (2)	Na1—O8ⁱⁱⁱ	2.437 (2)
In1—O3	2.255 (2)	Na1—O11ⁱ	2.462 (2)
In1—O8	2.338 (2)	Na1—O9ⁱⁱⁱ	2.476 (3)
In1—O7	2.356 (2)

O10—In1—O4	122.10 (9)	O8—In1—O7	55.29 (8)
O10—In1—O1	91.88 (9)	O12ⁱ—Na1—O2	99.82 (12)
O4—In1—O1	81.77 (10)	O5ⁱⁱ—Na1—O2	88.19 (8)
O10—In1—O6	164.80 (9)	O12ⁱ—Na1—O8ⁱⁱⁱ	110.79 (10)
O4—In1—O6	73.05 (8)	O5ⁱⁱ—Na1—O8ⁱⁱⁱ	77.75 (9)
O1—In1—O6	91.77 (10)	O2—Na1—O8ⁱⁱⁱ	85.24 (10)
O10—In1—O3	83.36 (9)	O12ⁱ—Na1—O11ⁱ	66.95 (9)
O1—In1—O3	72.36 (9)	O5ⁱⁱ—Na1—O11ⁱ	103.98 (11)
O6—In1—O3	83.70 (9)	O2—Na1—O11ⁱ	98.95 (12)
O10—In1—O8	93.10 (8)	O8ⁱⁱⁱ—Na1—O11ⁱ	175.47 (11)
O6—In1—O8	75.68 (8)	O12ⁱ—Na1—O9ⁱⁱⁱ	84.43 (10)
O3—In1—O8	74.12 (8)	O5ⁱⁱ—Na1—O9ⁱⁱⁱ	92.82 (11)
O10—In1—O7	87.13 (9)	O8ⁱⁱⁱ—Na1—O9ⁱⁱⁱ	65.13 (8)
O4—In1—O7	81.37 (9)	O11ⁱ—Na1—O9ⁱⁱⁱ	110.47 (11)
O6—In1—O7	94.55 (9)

Symmetry codes: (i) −x+1, y+1/2, −z+1/2; (ii) x−1, y, z; (iii) −x+1, y−1/2, −z+1/2.

Hydrogen-bond geometry (Å, º) top

D—H···A	D—H	H···A	D···A	D—H···A
O3—H3···O2ⁱ	0.86 (4)	1.76 (4)	2.620 (3)	177 (4)
O6—H6···O5^iv	0.82 (4)	1.77 (4)	2.578 (4)	170 (4)
O9—H9···O10^v	0.83 (4)	2.26 (4)	3.087 (4)	173 (4)
O12—H12···O7^vi	0.87 (4)	2.05 (4)	2.916 (3)	173 (4)

Symmetry codes: (i) −x+1, y+1/2, −z+1/2; (iv) −x+2, y+1/2, −z+1/2; (v) x+1/2, −y+3/2, −z; (vi) x−1/2, −y+1/2, −z.

Acknowledgements

This work was support by the National Natural Science Foundation of China (grant No. 20901033), the Scientific Research Foundation for the Returned Overseas Chinese Scholars (SEM), the NSF of Jiangxi Provincial (grant No. 2009GZH0056) and the Project of Education Department of Jiangxi Province (grant Nos. GJJ10016 and GJJ11381).

References

Balboa, S., Castiñeiras, A., Herle, P. S. & Strähle, J. (2007). Z. Anorg. Allg. Chem. 633, 2420–2424. CrossRef CAS Google Scholar
Bombi, G. G., Corain, B., Sheikh-Osman, A. A. & Valle, G. C. (1990). Inorg. Chim. Acta, 171, 79–83. CAS Google Scholar
Brandenburg, K. (2005). DIAMOND. Version 3.0. Crystal Impact GbR, Bonn, Germany. Google Scholar
Bruker (2008). APEX2 and SAINT. Bruker AXS Inc., Madison, Wisconsin, USA. Google Scholar
Carballo, R., Covelo, B., Vázquez-López, E. M., Castiñeiras, A. & Niclós, J. (2002). Z. Anorg. Allg. Chem. 628, 468–472. Web of Science CSD CrossRef CAS Google Scholar
Chen, W.-X., Ren, Y.-P., Long, L.-S., Huang, R.-B. & Zheng, L.-S. (2009). CrystEngComm, 11, 1522–1525. CrossRef CAS Google Scholar
Chen, S. M., Zhang, J. & Bu, X. H. (2008). Inorg. Chem. 47, 5567–5569. Web of Science CSD CrossRef PubMed CAS Google Scholar
Flack, H. D. (1983). Acta Cryst. A39, 876–881. CrossRef CAS Web of Science IUCr Journals Google Scholar
Janiak, C. (2003). J. Chem. Soc. Dalton Trans. pp. 2781–2804. CrossRef Google Scholar
Kitagawa, S., Kitaura, R. & Noro, S. I. (2004). Angew. Chem. Int. Ed. 43, 2334–2375. Web of Science CrossRef CAS Google Scholar
Lin, Z., Slawin, A. M. Z. & Morris, R. E. (2007). J. Am. Chem. Soc. 129, 4880–4881. Web of Science CrossRef PubMed CAS Google Scholar
Lis, T. (1982). Acta Cryst. B38, 937–939. CSD CrossRef CAS Web of Science IUCr Journals Google Scholar
O'Keeffe, M., Eddaoudi, M., Li, H. L., Reineke, T. & Yaghi, O. M. (2000). J. Solid State Chem. 152, 3–20. Web of Science CrossRef CAS Google Scholar
Parnham, E. R. & Morris, R. E. (2007). Acc. Chem. Res. 40, 1005–1013. Web of Science CrossRef PubMed CAS Google Scholar
Qu, Z.-R., Ye, Q., Zhao, H., Fu, D.-W., Ye, H.-Y., Xiong, R.-G., Akutagawa, T. & Nakamura, T. (2008). Chem. Eur. J. 14, 3452–3456. CrossRef PubMed CAS Google Scholar
Reichert, W. M., Holbrey, J. D., Vigour, K. B., Morgan, T. D., Broker, G. A. & Rogers, R. D. (2006). Chem. Commun. pp. 4767–4779. Web of Science CSD CrossRef Google Scholar
Sheldrick, G. M. (1996). SADABS. University of Göttingen, Germany. Google Scholar
Sheldrick, G. M. (2008). Acta Cryst. A64, 112–122. Web of Science CrossRef CAS IUCr Journals Google Scholar
Xu, L., Choi, E.-Y. & Kwon, Y.-U. (2007). Inorg. Chem. 46, 10670–10680. Web of Science CSD CrossRef PubMed CAS Google Scholar
Zhang, J., Chen, S. M. & Bu, X. H. (2008). Angew. Chem. Int. Ed. 47, 5434–5437. CrossRef CAS Google Scholar
Zhang, N., Liu, Q.-Y., Wang, Y.-L., Shan, Z.-M., Yang, E.-L. & Hu, H.-C. (2010). Inorg. Chem. Commun. 13, 706–710. Web of Science CSD CrossRef CAS Google Scholar

© International Union of Crystallography. Prior permission is not required to reproduce short quotations, tables and figures from this article, provided the original authors and source are cited. For more information, click here.

STRUCTURAL
CHEMISTRY

ISSN: 2053-2296

Volume 67| Part 5| May 2011| Pages m145-m148

doi:10.1107/S0108270111013606

Format		BIBTeX
		EndNote
		RefMan
		Refer
		Medline
		CIF
		SGML
		Plain Text
		Text

Format		BIBTeX
		EndNote
		RefMan
		Refer
		Medline
		CIF
		SGML
		Plain Text
		Text

Search term		doi		Advanced search
Author		volume	page

metal-organic compounds\(\def\hfill{\hskip 5em}\def\hfil{\hskip 3em}\def\eqno#1{\hfil {#1}}\)