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CAS Number: 1317-38-0
EC Number: 215-269-1
IUPAC name: Copper(II) oxide
APPLICATIONS
As a significant product of copper mining, copper(II) oxide is the starting point for the production of other copper salts.
For example, many wood preservatives are produced from copper oxide.
Copper(II) oxide is used as a pigment in ceramics to produce blue, red, and green, and sometimes gray, pink, or black glazes.
Copper(II) oxide is incorrectly used as a dietary supplement in animal feed.
Due to low bioactivity, negligible copper is absorbed.
Copper(II) oxide is used when welding with copper alloys.
A copper oxide electrode formed part of the early battery type known as the Edison–Lalande cell.
Copper oxide was also used in a lithium battery type (IEC 60086 code "G").
Copper(II) oxide is Used as moderate blue coloring agent in blue flame compositions with additional chlorine donors and oxidizers such as chlorates and perchlorates. Providing oxygen it can be used as flash powder oxidizer with metal fuels such as magnesium, aluminium, or magnalium powder.
Sometimes Copper(II) oxide is is used in strobe effects and thermite compositions as crackling stars effect.
Copper(II) oxide is used as a precursor in many copper-containing products such as wood preservatives and ceramics.
Copper Oxide (CuO) is a highly insoluble thermally stable copper source suitable for glass, optic and ceramic applications.
Copper(II) oxide is used As a pigment, in sweeting petroleum gases, in galvanic electrodes, metallurgical flux, as an optical glass polishing agent, and as a catalyst in organic reactions.
Copper(II) oxide is used as an adsorbent and absorbent, pigment, antifouling agent, wood preservative, optical glass polishing agent, welding flux for bronze materials, agricultural chemical and abrasive.
Copper(II) oxide is used in the preparation of intermediates, oxidizing/reducing agents, surface treating agents and process regulators.
Copper(II) oxide finds use in the manufacture of rayons, phosphors, and dry battery cells.
Copper(II) oxide serves as a catalyst in certain chemical reactions of industrial importance.
Copper(II) oxide is also employed in chemical sensors and superconducting materials.
Hazardous materials like cyanides, dioxins and halogenated hydrocarbons can be disposed through oxidation with copper oxide.
Copper(II) oxide is used as a pigment in ceramics to produce blue, red, and green (and sometimes gray, pink, or black) glazes.
Copper(II) oxide is also used to produce cuprammonium hydroxide solutions, used to make rayon.
Also, Copper(II) oxide is occasionally used as a dietary supplement in animals, against copper deficiency.
Copper (II) oxide has application as a p-type semiconductor, because it has a narrow band gap of 1.2 eV.
In addition, Copper(II) oxide is an abrasive used to polish optical equipment. Cupric oxide can be used to produce dry cell batteries.
Copper(II) oxide has also been used in wet cell batteries as the cathode, with lithium as an anode, and Dioxalane mixed with Lithium Perchlorate as the electrolyte.
Copper Oxide can be used to produce other copper salts.
Moreover, Copper(II) oxide is used when welding with copper alloys.
Another use for cupric oxide is as a substitute for iron oxide in thermite.
This can turn the thermite from an incendiary to a low explosive.
Copper(II) oxide is used as pigment in ceramics and fungicide
Also, copper(II) oxide is rarely used as a dietary supplement in animals
Copper(II) oxide has application as a p-type semiconductor due to its narrow band gap
In addition, copper(II) oxide is used to produce dry cell batteries/wet cell batteries
Copper(II) oxide is used as an alternative for iron oxide in thermite.
For Building copper-based structures copper(II) oxide is used.
These structures gradually change color due to oxidation.
To produce photoelectric cells in solar panels due to its efficient electrical conductivity properties copper(II) oxide is used.
Copper(II) oxide is used for Agricultural use to remove fungicides and pesticides.
Copper (II) oxide is occasionally used to rinse the glass.
Copper(II) oxide is used as a solvent of chromic iron minerals.
Various colors, including blue, green, red can be produced from Copper(II) oxide.
Also, Copper(II) oxide is used to pigment crystals or ceramic dye.
Copper(II) oxide is used as an insecticide and fumigant due to its fungicidal and microbicidal properties.
In addition to these, Copper(II) oxide is a precursor to make rayon.
Copper(II) oxide is also used as an abrasive to polish optical equipment.
Copper(II) oxide is used as a desulfurizing agent for petroleum gases and oils.
Another use that has been given to copper (II) oxide is to administer it orally in the form of needles or capsules of copper oxide wire to sheep and goats to control the gastrointestinal worms of cattle.
The copper(II) oxide is useful in industries such as:
•Agricultural
•Electroplating
•Non-Metallic Coatings
•Basic Chemicals
•Glass and Ceramics
•Electrical
•Analytical Reagents
DESCRIPTION
Copper(II) oxide or cupric oxide is an inorganic compound with the formula CuO.
A black solid, Copper(II) oxide is one of the two stable oxides of copper, the other being Cu2O or copper(I) oxide (cuprous oxide).
As a mineral, it is known as tenorite.
Copper(II) oxide is a product of copper mining and the precursor to many other copper-containing products and chemical compounds.
Copper(II) oxide may be found in over-the-counter vitamin-mineral supplements as a source of [DB09130].
The mean daily dietary intake of copper in adults ranges between 0.9 and 2.2 mg.
Common routes of Copper(II) oxide exposure include ingestion, dermal exposure and inhalation.
Copper(II) oxide nanoparticles (NPCuO) have industrial applications as antimicrobial agents in textiles and paints, and catalysts in organic synthesis.
They may also be produced from electronic wastes.
Copper(II) oxide poses potential health and environmental concern due to toxic and mutagenic particles generating reactive oxygen species.
Copper(II) oxide is a metal oxide that has the formula CuO.
Copper(II) oxide has an ionic structure.
Copper(II) oxide contains a copper(2+).
Copper(II) oxide is a black solid known as tenorite in mineral form, Copper(II) oxide can be formed by heating copper in the presence of oxygen.
Oxide compounds are not conductive to electricity.
However, certain perovskite structured oxides are electronically conductive finding application in the cathode of solid oxide fuel cells and oxygen generation systems. They are compounds containing at least one oxygen anion and one metallic cation.
They are typically insoluble in aqueous solutions (water) and extremely stable making them useful in ceramic structures as simple as producing clay bowls to advanced electronics and in light weight structural components in aerospace.
High Purity (99.999%) Copper(II) oxide Powder and electrochemical applications such as fuel cells in which they exhibit ionic conductivity.
Metal oxide compounds are basic anhydrides and can therefore react with acids and with strong reducing agents in redox reactions.
Copper(II) oxide is also available in pellets, pieces, powder, sputtering targets, tablets, and nanopowder.
Copper(II) oxide is generally immediately available in most volumes.
Cupric oxide, or copper (II) oxide, is an inorganic compound with the chemical formula CuO.
Copper(II) oxide is used as a precursor in many copper-containing products such as wood preservatives and ceramics.
Copper(II) oxide may be found in over-the-counter vitamin-mineral supplements as a source of Copper.
The mean daily dietary intake of copper in adults ranges between 0.9 and 2.2 mg 3.
Common routes of Copper(II) oxide exposure include ingestion, dermal exposure and inhalation.
Copper(II) oxide nanoparticles (NPCuO) have industrial applications as antimicrobial agents in textiles and paints, and catalysts in organic synthesis 1.
They may also be produced from electronic wastes.
Copper(II) oxide poses potential health and environmental concern due to toxic and mutagenic particles generating reactive oxygen species 1.
Copper(II) oxide occurs in nature in the minerals tenorite, melaconite, and paramelaconite.
In pure form, copper(II) oxide is a black to brownish powder or crystalline material.
Like copper(I) oxide, copper(II) oxide is a semiconductor, a material that conducts an electric current, although not nearly as well as conductors such as gold, silver, and aluminum.
Copper(II) oxide forms naturally in the Earth as a result of the weathering of copper sulfides (Cu2S and CuS).
Copper(II) oxide is prepared synthetically by heating copper metal in air to about 800°C (1,500°F) or, more commonly, by heating copper(II) carbonate (CuCO3) or copper(II) nitrate [Cu(NO3)2] to red heat.
Just under 0.007% of Earth's crust is comprised of copper.
Around 46% of Earth's crust is oxygen, and just over 20% of Earth's atmosphere is oxygen.
These two elements can come together chemically to form copper(II) oxide.
Copper (II) oxide is a higher oxide of copper and belongs to the monoclinic crystal system.
Copper (II) oxide occurs as a black solid with an ionic structure that melts above 1200°C with some loss of oxygen.
Also, Copper (II) oxide is an irritant, and causes damage to the central nervous system and endocrine system.
Copper (II) oxide can be formed by heating copper in air.
Copper(II) oxide is also called cupric oxide (CuO), which exists in nature in the form of a black or gray mineral called tenorite.
Also, Copper(II) oxide exists in black solid form and its melting temperature is higher than 1200 °C.
Copper(II) oxide is largely insoluble in solvents but it can react with acids to form copper salts.
Like cuprous oxide, copper (II) oxide can be manufactured by heating elemental (metallic) copper but at lower temperatures.
This method of production generates an impure form of the oxide; however, there are alternative ways of obtaining, for example, by heating some oxygen-containing copper compounds such as carbonate, hydroxide or nitrate.
PRODUCTION
Copper(II) oxide is produced on a large scale by pyrometallurgy, as one stage in extracting copper from its ores.
The ores are treated with an aqueous mixture of ammonium carbonate, ammonia, and oxygen to give copper(I) and copper(II) ammine complexes, which are extracted from the solids. These complexes are decomposed with steam to give CuO.
Copper(II) oxide can be formed by heating copper in air at around 300–800°C:
2 Cu + O2 → 2 CuO
For laboratory uses, pure copper(II) oxide is better prepared by heating copper(II) nitrate, copper(II) hydroxide, or basic copper(II) carbonate:
2 Cu(NO3)2(s) → 2 CuO(s) + 4 NO2(g) + O2(g) (180°C)
CuCO3(s) → CuO(s) + CO2(g)
Cu(OH)2(s) → CuO(s) + H2O(g)
REACTIONS
Copper(II) oxide dissolves in mineral acids such as hydrochloric acid, sulfuric acid or nitric acid to give the corresponding copper(II) salts:
CuO + 2 HNO3 → Cu(NO3)2 + H2O
CuO + 2 HCl → CuCl2 + H2O
CuO + H2SO4 → CuSO4 + H2O
Copper(II) oxide reacts with concentrated alkali to form the corresponding cuprate salts:
2 MOH + CuO + H2O → M2[Cu(OH)4]
Copper(II) oxide can also be reduced to copper metal using hydrogen, carbon monoxide, or carbon:
CuO + H2 → Cu + H2O
CuO + CO → Cu + CO2
2 CuO + C → 2Cu + CO2
PHYSICAL PROPERTIES
Copper(II) oxide belongs to the monoclinic crystal system.
The copper atom is coordinated by 4 oxygen atoms in an approximately square planar configuration.
The work function of bulk CuO is 5.3 eV.
Copper oxide is a dark grey powder with no characteristic odour and a molecular weight of 79.55 g/mol.
Copper(II) oxide has a relative density of 1.018 and a melting point of 1446°C.
Its vapour pressure is not measurable due to its high melting point.
Copper(II) oxide is slightly soluble in water (solubility in water at pH 6 (at 20°C) = 3.94 x 10-4 g/L).
Also, Copper(II) oxide is neither flammable nor explosive nor oxidizing.
-Chemical formula: CuO
-Molar mass: 79.545 g/mol
-Appearance: black to brown powder
-Density: 6.315 g/cm3
-Melting point: 1,326 °C (2,419 °F; 1,599 K)
-Boiling point: 2,000 °C (3,630 °F; 2,270 K)
-Solubility in water: insoluble
-Solubility: soluble in ammonium chloride, potassium cyanide
-insoluble in: alcohol, ammonium carbonate
Copper(II) Oxide Formula
The chemical combination of a metal and a non-metal generates an ionic compound.
We can determine the formula for an ionic compound based on how many electrons the metal atom loses and how many electrons the non-metal atom gains.
The Roman numeral II tells us the electric charge, or oxidation state, of the copper ion, which is +2.
This means each copper atom loses two electrons to form the ion Cu+2.
Oxygen is a non-metal and will always gain two electrons, giving it the oxidation state -2.
Since each oxygen atom has two extra electrons, the oxide ion is formed, which is O-2.
All ionic compounds have to be electrically neutral, which means the ratio of each element in the compound must contribute enough charge to cancel the charge of the other ion.
In the case of the copper(II) ion and the oxygen ion, we can see both ions have equal and opposite charges.
This means we only need one of each ion to form the neutral compound copper(II) oxide, which is CuO.
SYNONYMS
Cu(II) oxide
copper;oxygen(2-)
1344-70-3
CHEBI:75955
EINECS 215-706-6
Copper monoxide
Cupric oxide
Copporal, Oxocopper
Copper Brown
Black copper oxide
Paramelaconite
Ketocopper
BCO
