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Oxalate (systematic IUPAC name: ethanedioate) is an anion with the chemical formula C 2 O 2− 4.This dianion is colorless. It occurs naturally, including in some foods. It forms a variety of salts, for example sodium oxalate (Na 2 C 2 O 4), and several esters such as dimethyl oxalate ((CH 3) 2 C 2 O 4).
Gadolinium oxalate is the oxalate of gadolinium, with the chemical formula Gd 2 (C 2 O 4) 3. Its hydrate can be prepared by the reaction of gadolinium nitrate and oxalic acid . [ 1 ]
Gallium trichloride is a common starting reagent for the formation of organogallium compounds, such as in carbogallation reactions. [15] Gallium trichloride reacts with lithium cyclopentadienide in diethyl ether to form the trigonal planar gallium cyclopentadienyl complex GaCp 3. Gallium(I) forms complexes with arene ligands such as ...
Chemical formula Synonyms CAS number Ac 2 O 3: actinium(III) oxide: 12002-61-8 AgBF 4: Silver tetrafluoroborate: 14104-20-2 AgBr: silver bromide: 7785-23-1 AgBrO: silver hypobromite
In chemistry, an oxocarbon anion is a negative ion consisting solely of carbon and oxygen atoms, and therefore having the general formula C x O n− y for some integers x, y, and n. The most common oxocarbon anions are carbonate, CO 2− 3, and oxalate, C 2 O 2− 4. There are however a large number of stable anions in this class, including ...
It is a reducing agent [9] and its conjugate bases hydrogen oxalate (HC 2 O − 4) and oxalate (C 2 O 2− 4) are chelating agents for metal cations. It is used as a cleaning agent, especially for the removal of rust, because it forms a water-soluble ferric iron complex, the ferrioxalate ion.
The oxide ions are in a distorted cubic closest packing arrangement, and the gallium (III) ions occupy distorted tetrahedral and octahedral sites, with Ga–O bond distances of 1.83 and 2.00 Å respectively. [31] α-Ga 2 O 3 has the same structure as α-Al 2 O 3, wherein Ga ions are 6-coordinate. [32] [33]
Metal oxalate complexes are photoactive, degrading with loss of carbon dioxide. This reaction is the basis of the technique called actinometry. Ferrioxalate undergoes photoreduction. The iron centre is reduced (gains an electron) from the +3 to the +2 oxidation state, while an oxalate ion is oxidised to carbon dioxide: 2 [Fe(C 2 O 4) 3] 3− ...