A black solid, it is one of the two stable oxides of copper, the other being Cu 2 O or copper(I) oxide (cuprous oxide). Cu2O degrades to copper(II) oxide in moist air. (If an element does not have a prefix, assume that the subscript is “1.” Third, apply the above naming scheme. The copper atom is coordinated by 4 oxygen atoms in an approximately square planar configuration. The effect of hydrostatic pressure on the ambient temperature structure of CuO, Forsyth J.B., Hull S., J. No predicted properties have been calculated for this compound. As a mineral, it is known as tenorite. The resulting compound carries a neutral electrical charge. It is produced on a large scale by pyrometallurgy, as one stage in extracting copper from its ores. Formation of copper(I) oxide is the basis of the Fehling's test and Benedict's test for reducing sugars. 129, 12 (1999) 2278-2279, National Institute for Occupational Safety and Health, Ullmann's Encyclopedia of Industrial Chemistry, "Uses of Copper Compounds: Other Copper Compounds", National Pollutant Inventory - Copper and compounds fact sheet, CDC - NIOSH Pocket Guide to Chemical Hazards, https://en.wikipedia.org/w/index.php?title=Copper(II)_oxide&oldid=982213512, Chemical articles with multiple compound IDs, Multiple chemicals in an infobox that need indexing, Pages using collapsible list with both background and text-align in titlestyle, Articles containing unverified chemical infoboxes, Creative Commons Attribution-ShareAlike License, This page was last edited on 6 October 2020, at 20:09. [1], The work function of bulk CuO is 5.3 eV[5], As a significant product of copper mining, copper(II) oxide is the starting point for the production of other copper salts. A copper oxide electrode formed part of the early battery type known as the Edison–Lalande cell. Salts are hygroscopic, or tend to pick up water. Copper(I) oxide is found as the reddish mineral cuprite. Phys. For CuO use the hints and resources below to help write the name. It can be shown using Cu2O that the Kramers–Kronig relations do not apply to polaritons.[11]. It is a product of copper mining and the precursor to many other copper-containing products and chemical compounds.[3]. The ionic compound Cu2O is named copper I oxide. CopyCopied, Validated by Experts, Validated by Users, Non-Validated, Removed by Users, Predicted data is generated using the ACD/Labs Percepta Platform - PhysChem Module. Copper(I) oxide is also responsible for the pink color in a positive Benedict's test. Except where otherwise noted, data are given for materials in their, L. O. Grondahl, Unidirectional current carrying device, Patent, 1927. Cu2O crystallizes in a cubic structure with a lattice constant al=4.2696 Å. Copper(II) oxide belongs to the monoclinic crystal system. Steps to Naming Covalent Compounds. [7], It is also used when welding with copper alloys.[8]. Apply the rules for naming that type of compound. Another unusual feature of the ground state excitons is that all primary scattering mechanisms are known quantitatively. Dilute sulfuric acid and nitric acid produce copper(II) sulfate and copper(II) nitrate, respectively.[5]. In the history of semiconductor physics, Cu2O is one of the most studied materials, and many experimental semiconductor applications have been demonstrated first in this material: The lowest excitons in Cu2O are extremely long lived; absorption lineshapes have been demonstrated with neV linewidths, which is the narrowest bulk exciton resonance ever observed. Any copper oxide in which the metal is in the +1 oxidation state. For example, many wood preservatives are produced from copper oxide.[3]. In terms of their coordination spheres, copper centres are 2-coordinated and the oxides are tetrahedral. CopyCopied, InChI=1S/2Cu.O/q2*+1;-2 J. Brandt, D. Fröhlich, C. Sandfort, M. Bayer, H. Stolz, and N. Naka. Copper(II) oxide or cupric oxide is the inorganic compound with the formula CuO. [6] Due to low bioactivity, negligible copper is absorbed. For example, table salt, or sodium chloride, consists of the Na + cation bonded to the Cl-anion to form NaCl.

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