The structure of <i>trans</i>-diaquabis[(±)-hydrogen malato]cobalt(II) dihydrate

Karipides, A.

doi:10.1107/s0567740881005190

Cited by 15 publications

(2 citation statements)

References 6 publications

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“…The Co−O bond distances are in the range from 2.049(2) to 2.091(2) Å for 1 and 2.041(2) to 2.125(2) Å for 2 . These are comparable with corresponding distances in complexes (NH 4 ) 4 [Co(C 6 H 5 O 7 ) 2 ] (2.051(2)−2.157(2) Å) ( 4 ), K 2 [Co 2 (C 6 H 5 O 7 ) 2 (H 2 O) 4 ]·6H 2 O (2.042(2)−2.194(2) Å) ( 5 ), Na 2 [Co 2 (C 6 H 5 O 7 ) 2 (H 2 O) 4 ]·6H 2 O (2.044(2)−2.169(2) Å) ( 6 ), [Co(C 4 H 5 O 5 ) 2 (H 2 O) 2 ]·2H 2 O (2.066(1)−2.112(1) Å) ( 7 ), and [Co(CO 2 CH 2 CH(OH)CO 2 )]·3H 2 O (2.067(3)−2.136(3) Å) ( 8 ) …”

Section: Resultssupporting

confidence: 72%

pH-Dependent Syntheses, Structural and Spectroscopic Characterization, and Chemical Transformations of Aqueous Co(II)−Quinate Complexes: An Effort to Delve into the Structural Speciation of the Binary Co(II)−Quinic Acid System

et al. 2009

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Cobalt(II) is an essential metal ion, which can react with biologically relevant substrates in aqueous media, affording discrete soluble forms. D-(-)-quinic acid is a representative metal ion binder, capable of promoting reactions with Co(II) under pH-specific conditions, leading to the isolation of the new species K[Co(C(7)H(11)O(6))(3)] x 3 CH(3)CH(2)OH (1), Na[Co(C(7)H(11)O(6))(3)] x 3 CH(3)CH(2)OH x 2.25 H(2)O (2), and [Co(C(7)H(11)O(6))(2)(H(2)O)(2)] x 3 H(2)O (3). Compounds 1-3 were characterized by elemental analysis, spectroscopic techniques (Fourier-transform infrared, UV-visible, electron paramagnetic resonance (EPR), electrospray ionization mass spectrometry), magnetic studies, and X-ray crystallography. Compound 1 crystallizes in the cubic space group P2(1)3, with a = 15.3148(19) A, V = 3592.0(8) A(3), and Z = 4. Compound 2 crystallizes in the orthorhombic space group P2(1)2(1)2(1), with a = 14.9414(8) A, b = 15.9918(9) A, c = 16.0381(9) A, V = 3832.1(4) A(3), and Z = 4. Compound 3 crystallizes in the monoclinic space group P2(1)/m, with a = 13.2198(10) A, b = 5.8004(6) A, c = 15.3470(12) A, beta = 108.430(7), V = 1116.45(17) A(3), and Z = 4. The lattices in 1-3 reveal the presence of mononuclear Co(II) units bound exclusively to quinate (1 and 2) or quinate and water ligands (3), thus projecting the unique chemical reactivity in each investigated system and suggesting that 3 is an intermediate in the synthetic pathway leading to 1 and 2. The octahedral sites of Co(II) are occupied by oxygens, thereby reflecting the nature of interactions between the divalent metal ion and quinic acid. The magnetic and EPR data on 1 and 3 support the presence of a high-spin octahedral Co(II) in an oxygen environment, having a ground state with an effective spin of S = 1/2. The significance of 3 is further reflected into the aqueous speciation of the binary Co(II)-quinic acid system, in which 3 appears as a competent participant linked to the solid state species 1. The physicochemical profiles of 1-3, in the solid state and in solution, earmark the importance of aqueous structural speciation, which projects chemical reactivity pathways in the binary Co(II)-quinate system, involving soluble Co(II) forms emerging through interactions with low molecular mass O-containing physiological substrates, such as quinic acid.

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Section: Resultssupporting

confidence: 72%

pH-Dependent Syntheses, Structural and Spectroscopic Characterization, and Chemical Transformations of Aqueous Co(II)−Quinate Complexes: An Effort to Delve into the Structural Speciation of the Binary Co(II)−Quinic Acid System

et al. 2009

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“…The other Co−O distances in 2 − 4 are in the normal range, which are similar to those observed in the other cobalt(II) citrate complexes. ,,, Moreover, these Co−O distances are also comparable to those in the other cobalt(II) hydroxycarboxylate complexes. Such as [Co( S -Hmal)(H 2 O) 2 ] n ·2 n H 2 O [2.067(3)−2.136(3) Å], trans -[Co( R , S -H 2 mal) 2 (H 2 O) 2 ]·2H 2 O [2.066(1)−2.112(1) Å] (H 3 mal = malic acid), [Co 2 ( R , R -H 2 tart) 2 (H 2 O) 2 ] n ·3 n H 2 O [2.04(1)−2.16(1) Å] (H 4 tart = tartaric acid), [Co(Hglyc) 2 ] n [2.053(1)−2.118(1) Å] (H 2 glyc = glycolic acid), [Co( R , S -Hlact) 2 (H 2 O) 2 ]·H 2 O [2.018(3)−2.129(3) Å] (H 2 lact = lactic acid), and [Co[CO 2 C(OH)(CH 3 ) 2 ] 2 (H 2 O) 2 ] [2.023(2)−2.090(2) Å] . The Co1−Co1i distance in 2 is 5.348(1) Å, which is very similar to those observed in K 2 [Co 2 (Hcit) 2 (H 2 O) 4 ]·6H 2 O [5.247(1) Å], Na 2 [Co 2 (Hcit) 2 (H 2 O) 4 ]·6H 2 O [5.361(1) Å], K 2 [Ni 2 (Hcit) 2 (H 2 O) 4 ]·6H 2 O [5.364(1) Å], and Co 3 (Hcit) 2 (4,4‘-bpy) 4 (H 2 O) 2 ·4H 2 O [5.378(1) Å] (bpy = 4,4‘- bipyridine) 26 but is longer than that observed in 4 [4.955(2) Å].…”

Section: Resultsmentioning

confidence: 99%

Structural Diversities of Cobalt(II) Coordination Polymers with Citric Acid

Zhou

Deng

Wan

2005

Crystal Growth & Design

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The reactions of cobalt(II) ion with citric acid (C 6 H 8 O 7 ) H 4 cit) have been studied in an acidic aqueous solution of pH 1-4, which result in the isolations of four new polymeric cobalt(II) citrate complexes:The complexes have been characterized by spectroscopic and single crystal X-ray diffraction studies. The Co(II) ion in each complex exists in an octahedral coordination environment. The citrate ligand binds the Co(II) ion tridentately via its R-hydroxyl, R-carboxylate, and one of the β-carboxylate groups as a basic feature. The polymeric structures are constructed by the further coordination of R-carboxylate or β-carboxylate groups. Complex 1 forms a chiral helical chain running along the a-axis of the crystal via the two bridged bonded oxygen atoms of the R-carboxylate group, leaving the β-carboxylic acid group free and forming strong hydrogen bond. The dimeric cobalt-(II) citrate unit [Co 2 (Hcit) 2 (H 2 O) 4 ] 2in the complex 2 forms a one-dimensional polymeric chain through the coupling of long-arm β-carboxylate groups with the planar [Co(H 2 O) 4 ] and [Co 2 (Hcit) 2 (H 2 O) 4 ] units. The [Co(Hcit)(H 2 O)]unit in complex 3 forms an infinite chain along a 2 1 axis. Complex 4 forms a layered complex through the links of the new dimeric unit [Co 2 (Hcit) 2 (H 2 O) 2 ] by the oxygen atoms of the β-carboxylate groups. Interconversions between 1, 3, and 4 are found to be pH-and counterion-dependent. Heating of coordination polymer 2 results in the irreversible formation of 3. The structural diversities of these cobalt(II) citrate polymers demonstrate that pH, counterions, and reaction temperature play essential roles in the formations of such one-dimensional and two-dimensional frameworks.

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The Interaction of α-Hydroxycarboxylic Acids with Metal Ions: Lactic Acid (H2L1) and 2-Methyllactic Acid (H2L2) with Cobalt(II) Crystal and Molecular Structures of [Co(HL1)2(H2O)2]·H2O and [Co(HL2)2(H2O)2]

Carballo

Covelo

Vázquez‐López

et al. 2002

Z. anorg. allg. Chem.

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The cobalt(II) complexes [Co(HL 1 ) 2 (H 2 O) 2 ]·H 2 O) (1) and [Co(HL 2 ) 2 (H 2 O) 2 ] (2) [(HL 1 ) Ϫ ϭ (±)-lactate, (HL 2 ) Ϫ ϭ 2-Methyllactate] were prepared and characterized structurally. The cobalt atom is in a distorted octahedral environment in both compounds. Both α-hydroxycarboxylato ligands are O,O'-bidentate chelating monoanions. The presence of a lattice water molecule in 1 makes its

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The structure of trans-diaquabis[(±)-hydrogen malato]cobalt(II) dihydrate

Abstract: Abstract. 1Co{(_)-

Cited by 15 publications

References 6 publications

pH-Dependent Syntheses, Structural and Spectroscopic Characterization, and Chemical Transformations of Aqueous Co(II)−Quinate Complexes: An Effort to Delve into the Structural Speciation of the Binary Co(II)−Quinic Acid System

pH-Dependent Syntheses, Structural and Spectroscopic Characterization, and Chemical Transformations of Aqueous Co(II)−Quinate Complexes: An Effort to Delve into the Structural Speciation of the Binary Co(II)−Quinic Acid System

Structural Diversities of Cobalt(II) Coordination Polymers with Citric Acid

The Interaction of α-Hydroxycarboxylic Acids with Metal Ions: Lactic Acid (H2L1) and 2-Methyllactic Acid (H2L2) with Cobalt(II) Crystal and Molecular Structures of [Co(HL1)2(H2O)2]·H2O and [Co(HL2)2(H2O)2]

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