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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.
Copper oxide is any of several binary compounds composed of the elements copper and oxygen. Two oxides are well known, Cu 2 O and CuO, corresponding to the minerals cuprite and tenorite, respectively. Paramelaconite (Cu 4 O 3) is less well characterized. [1] Copper oxide may refer to: Copper(I) oxide (cuprous oxide, Cu 2 O) Copper(II) oxide ...
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.
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 ...
They are very reactive towards oxygen to form copper(I) oxide and have many uses in chemistry. They are synthesized by treating copper(I) compounds with Grignard reagents , terminal alkynes or organolithium reagents ; [ 12 ] in particular, the last reaction described produces a Gilman reagent .
For acetone dipole-dipole interactions are a major driving force behind the structure of its crystal lattice. The negative dipole is caused by oxygen. Oxygen is more electronegative than carbon and hydrogen, [13] causing a partial negative (δ-) and positive charge (δ+) on the oxygen and remainder of the molecule, respectively.
Yttrium barium copper oxide (YBCO) is a family of crystalline chemical compounds that display high-temperature superconductivity; it includes the first material ever discovered to become superconducting above the boiling point of liquid nitrogen [77 K (−196.2 °C; −321.1 °F)] at about 93 K (−180.2 °C; −292.3 °F).
Given nitrate's low basicity, the tendency of metal nitrate complexes toward hydrolysis is expected. 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