Copper(II) oxalate obtained through the reaction of 1,2-ethanediol with Cu(NO3)2·3H2O

Bîrzescu, M.; Niculescu, Mircea; Dumitru, Raluca; Budrugeac, P.; Segal, E.

doi:10.1007/s10973-007-8599-1

Cited by 22 publications

(10 citation statements)

References 27 publications

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“…The bending vibration of crystal water is very likely responsible for the very broad band in the commercial sample that is nominally a copper(II) oxalate hemihydrate (Figure 2c). Such broad bands were also reported previously, 12,20,24 but unfortunately the most comprehensive study of the vibrational spectra of copper(II) oxalate, presumably performed on a dihydrate, 21 only presented a list of wavenumbers with approximate intensity and not the infared spectrum itself so that a close comparison is difficult. The width of the band above 1600 cm −1 is reduced in the case of the precipitate obtained from ethanolic solution (Figure 2b).…”

Section: Resultssupporting

confidence: 67%

“…In analogy to the structure of HKUST-1 (Figure d) and other MOFs, one would expect a geometry in which the CC bond is oriented along to line connecting two Cu 2+ dimers, and consequently each carboxyl group binds to one of the two connected metal centers (Figure e). In contrast, the crystal structure of copper(II) oxalate has been proposed to consist of a coordination polymer, i.e., ribbons of alternating oxalate ions and metal ions, the latter being located “sideways” between the two carboxylate groups of the oxalate ions (Figure f) and surrounded by two such oxalate ions leading to a zigzag chain structure. − This structural motif is also encountered in other copper coordination polymers and oxalato complexes . Adjacent ribbons are perpendicular to each other in a fishbone arrangement allowing for additional coordinative interactions between oxalate ions of a specific ribbon and Cu 2+ ions of the next ribbon, thus stabilizing the structure …”

Section: Introductionmentioning

confidence: 99%

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Formation and Structure of Copper(II) Oxalate Layers on Carboxy-Terminated Self-Assembled Monolayers

et al. 2014

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Copper(II) oxalate was grown on carboxy-terminated self-assembled monolayers using a step-by-step approach by dipping the surfaces alternately in ethanolic solutions of copper(II) acetate and oxalic acid with intermediate thorough rinsing steps. The deposition was monitored by reflection absorption infrared spectroscopy (RAIRS), a quartz microbalance with dissipation measurement (QCM-D), scanning electron microscopy (SEM), and helium ion microscopy (HIM). Amounts of material corresponding to a coverage of 75% of a monolayer are deposited in each dipping step in copper(II) acetate solution while deposition of oxalic acid produces a viscoelastic layer that is partially removed by rinsing. This points toward initial aggregation but acid not bound to Cu(2+) ions as oxalate ions is removed by the rinsing steps. RAIRS further indicates that the material grows as copper(II) oxalate ribbons similar to the crystal structure but with ribbons oriented roughly parallel to the surface. SEM and HIM give evidence of the formation of needle-shaped structures which are a possible explanation for the viscoelastic behavior of the layer.

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Section: Resultssupporting

confidence: 67%

Section: Introductionmentioning

confidence: 99%

Formation and Structure of Copper(II) Oxalate Layers on Carboxy-Terminated Self-Assembled Monolayers

et al. 2014

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“…Upon evaporation of a highly concentrated solution of Cu(NO 3 ) 2 · 3H 2 O in EG (molar ratio 1:2 to 1:3) at room temperature, as done by Knetsch and Groeneveld , basic copper nitrate, Cu 2 (OH) 3 (NO 3 ), and copper oxalate, CuC 2 O 4 , were formed after some days. The oxidation of EG to oxalate is due to the oxidizing potential of nitrate ions . Light blue crystals of 8 could only be grown when the solution was stored at 4 °C.…”

Section: Resultsmentioning

confidence: 99%

“…The oxidation of EG to oxalate is due to the oxidizing potential of nitrate ions. [36] Light blue crystals of 8 could only be grown when the solution was stored at 4°C. A similar coordination was also found in the ethylene diamine analogue [Cu(en) 2 (NO 3 ) 2 ].…”

Section: [Cu(eg) 2 (No 3 ) 2 ] (8)mentioning

confidence: 99%

Influence of Common Anions on the Coordination of Metal Cations in Polyalcohols

Teichert

Ruck

2019

Eur J Inorg Chem

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Polyalcohols (polyols), such as ethylene glycol, have mild reducing ability. They are used in the so‐called polyol process to produce metallic nanoparticles of various kinds. In these syntheses, the effective reduction potential of the polyol strongly depends on the presence of other anions. Those anions compete against the polyol molecules for the direct bonding to the metal cations. As an indicator for the coordination behavior of polyols, we crystallized and structurally characterized 19 new coordination compounds with Mn, Co, Ni, Cu, Zn, Cd, Pb, or Bi. 15 of these compounds comprise nitrate ions, the others acetate ions. Compared to the already known chloride and sulfate analogues, nitrate shows an intermediate coordination affinity towards the metal cations considered here. While no direct metal–nitrate coordination occurs with Co2+, Ni2+, and Zn2+, mixed nitrate–polyol coordination environments are found for Mn2+, Cu2+, Cd2+, and Bi3+. Because of its strong chelating property, the acetate ion always coordinates the metal cation, competing with the polyol. The first mononuclear and dinuclear metal acetate diol coordination compounds were obtained with Co2+ and Cu2+, respectively. The coordination affinity of nitrate and acetate ligands in solid metal polyol complexes fully corresponds with our recent observations of the anion‐dependent reduction behavior of copper(II) salts in polyols.

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“…The IR spectrum of oxalate precursor (Figure 1a) reveals the presence of water [3410 cm −1 (ν OH , ν H2O ), 794 cm −1 (lattice water)] [41,54], oxalate anions [as bidentate ligand: 1642 cm −1 (ν asym (O=C-O) ) + δ sym (HOH), 1308 cm −1 (ν sym (O=C-O) , 1051 cm −1 (ν (C-O) )] [42]; as tetradentate ligand: 1445 cm −1 (ν sym (OCO) ), 915 cm −1 (δ (OCO) )] [55], and metal-oxygen linkages [600-400 cm −1 : ν (La-O) and ν (Fe-O) vibrations]. The IR spectra of LaFeO 3 obtained after calcination at 550 • C (Figure 1b) and 700 • C (Figure 1c) exhibit only the bands characteristic for vibrations ν(La-O) and ν(Fe-O) in the range of 600-400 cm −1 [43,44].…”

Section: Characterization Of Lafementioning

confidence: 99%

Lanthanum Ferrite Ceramic Powders: Synthesis, Characterization and Electrochemical Detection Application

et al. 2020

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The perovskite-type lanthanum ferrite, LaFeO3, has been prepared by thermal decomposition of in situ obtained lanthanum ferrioxalate compound precursor, LaFe(C2O4)3·3H2O. The oxalate precursor was synthesized through the redox reaction between 1,2-ethanediol and nitrate ion and characterized by chemical analysis, infrared spectroscopy, and thermal analysis. LaFeO3 obtained after the calcination of the precursor for at least 550–800 °C/1 h have been investigated by X-ray diffraction (XRD), field emission scanning electron microscopy (FE-SEM), transmission electron microscopy (TEM), and high-resolution transmission electron microscopy (HRTEM). A boron-doped diamond electrode (BDD) modified with LaFeO3 ceramic powders at 550 °C (LaFeO3/BDD) by simple immersion was characterized by cyclic voltammetry and tested for the voltammetric and amperometric detection of capecitabine (CCB), which is a cytostatic drug considered as an emerging pollutant in water. The modified electrode exhibited a complex electrochemical behaviour by several redox systems in direct relation to the electrode potential range. The results obtained by cyclic voltammetry (CV), differential-pulsed voltammetry (DPV), and multiple-pulsed amperometry proved the electrocatalytic effect to capecitabine oxidation and reduction and allowed its electrochemical detection in alkaline aqueous solution.

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Copper(II) oxalate obtained through the reaction of 1,2-ethanediol with Cu(NO3)2·3H2O

Cited by 22 publications

References 27 publications

Formation and Structure of Copper(II) Oxalate Layers on Carboxy-Terminated Self-Assembled Monolayers

Formation and Structure of Copper(II) Oxalate Layers on Carboxy-Terminated Self-Assembled Monolayers

Influence of Common Anions on the Coordination of Metal Cations in Polyalcohols

Lanthanum Ferrite Ceramic Powders: Synthesis, Characterization and Electrochemical Detection Application

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