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Copper nitrate, in combination with acetic anhydride, is an effective reagent for nitration of aromatic compounds, known as the Menke nitration. [17] Hydrated copper nitrate adsorbed onto clay affords a reagent called "Claycop". The resulting blue-colored clay is used as a slurry, for example for the oxidation of thiols to disulfides.
The nitrate salt of the acetonitrile complex, i.e., [Cu(MeCN) 4]NO 3, is generated by the reaction of silver nitrate with a suspension of copper metal in acetonitrile. [2] Cu + AgNO 3 + 4 CH 3 CN → [Cu(CH 3 CN) 4]NO 3 + Ag. Tertiary phosphine complexes of the type [Cu(P(C 6 H 5) 3) 3]NO 3 are prepared by the reduction of copper(II) nitrate by ...
Thus copper(II) nitrate readily dissociates in aqueous solution to give the aqua complex: Cu(NO 3) 2 + 6 H 2 O → [Cu(H 2 O) 6](NO 3) 2. Pyrolysis of metal nitrates yields oxides. [18] Ni(NO 3) 2 → NiO + NO 2 + 0.5 O 2. This reaction is used to impregnate oxide supports with nickel oxides. Nitrate reductase enzymes convert nitrate to
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The structure thus resembles in some sense the main polymorphs of SiO 2, but cuprous oxide's lattices interpenetrate. Cu 2 O crystallizes in a cubic structure with a lattice constant a l = 4.2696 Å. The copper atoms arrange in a fcc sublattice, the oxygen atoms in a bcc sublattice. One sublattice is shifted by a quarter of the body diagonal.
The copper-containing enzyme nitrite reductase (CuNIR) catalyzes the 1-electron reduction of nitrite to nitric oxide. The proposed mechanism entails the protonation of a κ 2O,O -NO 2 -Cu(I) complex. This protonation induces cleavage of an N–O bond, giving a HO–Cu–ON center, which features a nitric oxide ligand O-bonded to Cu(II) (an ...
In the NO − 3 anion, the oxidation state of the central nitrogen atom is V (+5). This corresponds to the highest possible oxidation number of nitrogen. Nitrate is a potentially powerful oxidizer as evidenced by its explosive behaviour at high temperature when it is detonated in ammonium nitrate (NH 4 NO 3), or black powder, ignited by the shock wave of a primary explosive.
It can be formed by heating copper in air at around 300–800 °C: 2 Cu + O 2 → 2 CuO. For laboratory uses, copper(II) oxide is conveniently prepared by pyrolysis of copper(II) nitrate or basic copper(II) carbonate: [4] 2 Cu(NO 3) 2 → 2 CuO + 4 NO 2 + O 2 (180°C) Cu 2 (OH) 2 CO 3 → 2 CuO + CO 2 + H 2 O. Dehydration of cupric hydroxide ...