COPPER OXIDE

CuO

CAS Number: 1317-38-0
EC Number: 215-269-1
Hill Formula: CuO
Molar Mass: 79.54 g/mol    

Copper oxide is a compound from the two elements copper and oxygen.

Copper oxide may refer to:
Copper(I) oxide (cuprous oxide, Cu2O)
Copper(II) oxide (cupric oxide, CuO)
Copper peroxide (CuO2)
Copper(III) oxide (Cu2O3)
Copper(IV) oxide (CuO2)

Copper oxide (CuO) is a semi-conducting compound with a monoclinic structure. 
CuO has attracted particular attention because Copper oxide is the simplest member of the family of copper compounds and exhibits a range of potentially useful physical properties, such as high temperature superconductivity, electron correlation effects, and spin dynamics. 

Copper oxide is relatively cheap, easily mixed with polarized liquids (i.e., water) and polymers, and relatively stable in terms of both chemical and physical properties. 
Highly ionic nanoparticulate metal oxides, such as CuO, may be particularly valuable antimicrobial agents as they can be prepared with extremely high surface areas and unusual crystal morphologies.

Copper oxide (CuO) nanoparticles have been characterized, both physically and chemically, and investigated with respect to potential antimicrobial applications. 
Copper oxide was found that nanoscaled CuO, as generated by thermal plasma technology, demonstrated particle sizes in the range 20–95 nm with a mean surface area of 15.7 m2/g. 

CuO nanoparticles in suspension showed activity against a range of bacterial pathogens, including MRSA and E. coli, with MBCs ranging from 0.1 to 5.0 mg/mL. 
As with silver, studies of CuO nanoparticles incorporated into polymers suggest that the release of ions may be required for optimum killing. 

Incorporation of nano-CuO into porous elastomeric polyurethane films has demonstrated potential for a number of applications. 
Studies have shown this approach to be effective against MRSA within 4 h of contact.

Cu2O (copper (I) oxide; cuprous oxide) is a red powder and can also be produced as nanoparticles. 
Similar activity to CuO (copper(II) oxide; cupric oxide) has been shown against a range of species and strains.

Copper oxides are unusual in two respects. 
First, octahedral-site CuII:t6e3 contains a single e hole in the 3d shell, which makes Copper oxide orbitally degenerate and therefore a strong Jahn–Teller ion; consequently, CuII ions normally occupy square coplanar, pyramidal, or octahedral sites that are deformed to tetragonal (c/a > 1) symmetry by Jahn–Teller orbital ordering. 

However, in the absence of a cooperativity that stabilizes long-range orbital ordering, the electrons may couple locally to E-mode vibrations, forming vibronic states in a dynamic Jahn–Teller coupling. 
Second, the CuII:3d9 energy level lies below the top of the O2 −:2p6 valence band in an ionic model; the introduction of covalent bonding creates states of e-orbital symmetry at the top of the O2 −:2p6 bands that have a large O-2pσ component. 

Locally this O-2pσ component increases dramatically on oxidation of CuII to CuIII. 
The change in orbital mixing represents a polarization of the oxygen atoms that decreases the equilibrium Cu-O bond length, but the change in polarization is fast relative to the motion of the oxygen nucleus. 

Therefore, a dynamic vibronic phenomenon may reflect coupling to the polarization cloud of the oxygen atoms rather than to significant oxygen-atom displacements. 
Nevertheless, hybridization of an atomic vibration wave with a polarization wave on the oxygen-atom array would significantly increase the effective mass m* of an itinerant electron.

The copper-oxide superconductors all contain CuO2 sheets in which any apical Cu-O bonds perpendicular to a sheet are significantly longer than the in-plane Cu-O bonds. 
This structural feature signals full occupancy of the (3z2–r2) orbitals of an e-orbital pair. 

On oxidation of the CuO2 sheets, the system undergoes a crossover from localized to itinerant electronic behavior, and a thermodynamically distinguishable p-type superconductive phase is found at crossover with a hole concentration x per Cu atom of the CuO2 sheets in the range 0.14 ≤ x ≤ 0.22. 
Superconductivity has also been observed on reduction of the CuO2 sheets, but n-type superconductivity is more difficult to stabilize and has been studied much less.

The potential of metallic copper as an intrinsically antibacterial material is gaining increasing attention in the face of growing antibiotics resistance of bacteria.
However, the mechanism of the so-called “contact killing” of bacteria by copper surfaces is poorly understood and requires further investigation. 

In particular, the influences of bacteria–metal interaction, media composition, and copper surface chemistry on contact killing are not fully understood. 
In this study, copper oxide formation on copper during standard antimicrobial testing was measured in situ by spectroscopic ellipsometry. 

In parallel, contact killing under these conditions was assessed with bacteria in phosphate buffered saline (PBS) or Tris-Cl. 
For comparison, defined Cu2O and CuO layers were thermally generated and characterized by grazing incidence X-ray diffraction. 

The antibacterial properties of these copper oxides were tested under the conditions used above. 
Finally, copper ion release was recorded for both buffer systems by inductively coupled plasma atomic absorption spectroscopy, and exposed copper samples were analyzed for topographical surface alterations. 

Copper oxide was found that there was a fairly even growth of CuO under wet plating conditions, reaching 4–10 nm in 300 min, but no measurable Cu2O was formed during this time. 
CuO was found to significantly inhibit contact killing, compared to pure copper. 

In contrast, thermally generated Cu2O was essentially as effective in contact killing as pure copper. 
Copper ion release from the different surfaces roughly correlated with their antibacterial efficacy and was highest for pure copper, followed by Cu2O and CuO. 

Tris-Cl induced a 10–50-fold faster copper ion release compared to PBS. 
Since the Cu2O that primarily forms on copper under ambient conditions is as active in contact killing as pure copper, antimicrobial objects will retain their antimicrobial properties even after oxide formation.

The most common forms of copper oxide are copper (I) oxide and copper (II) oxide. 
These forms of copper oxide as well as the other forms are formed when oxygen combines with copper in different ways.

Copper (I) oxide is a reddish powder whereas Copper (II) oxide is a black powder. 
These inorganic compounds occur naturally as minerals in the form of crystals. 
Both forms of copper oxide are used to produce pigments.

The “I” and “II” in copper oxide represents the number of electrons that the metal has provided when copper oxide is brought into contact with metal.

Some uses for copper oxide are:
Building copper-based structures. 
These structures gradually change color due to oxidation.

Producing photoelectric cells in solar panels due to Copper oxide efficient electrical conductivity properties.
Agricultural use to remove fungicides and pesticides.
Copper oxide can cause flulike symptoms and shortness of breath if ingested by humans.

Copper(I) Oxide is also called as cuprous oxide, an inorganic compound with the chemical formula Cu2O. 
Copper oxide is covalent in nature. 

Copper(I) oxide crystallizes in a cubic structure. 
Copper oxide is easily reduced by hydrogen when heated. 

Copper oxide undergoes disproportionation in acid solutions producing copper(II) ions and copper. 
When the cupric oxide is gently heated with metallic copper, Copper oxide is converted into cuprous oxide. 
Copper oxide acts as a good corrosion resistance, due to reactions at the surface between the copper and the oxygen in air to give a thin protective oxide layer.

Oxygen can be combined with copper in diverse ways to produce 2 kinds of compounds: copper oxide (I) that is a reddish powder and copper oxide (II), a black powder. 
These compounds are also found in nature as minerals, both copper oxides are used in the production of pigments independently, each has different uses.

Copper oxide, also called cuprous oxide (Cu2O), is found in nature in a mineral called cuprite, although most of the compound used at the industrial level is obtained synthetically. 
Industrially, Copper oxide can be formed by heating metallic copper at extreme temperatures or by electrolysis of saline solutions with the help of copper electrodes and by mixing some other copper composites with reducing agents.

Copper oxide is also called copper oxide (CuO), which exists in nature in the form of a black or gray mineral called tenorite. 
Copper oxide exists in black solid form and Copper oxide melting temperature is higher than 1200 °C. 
Copper (II) oxide is largely insoluble in solvents but Copper oxide 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.

Copper Oxide where copper is in liquid form is called cuprous oxide. 
Cu2O is the chemical structure of cuprous oxide. 

Well, here in Cu2O copper and oxygen share a covalent bond; hence Copper oxide naturally has covalent bonds. 
Crystals of cuprous oxide are found in cubic shape. 

When you heat the solution of Cu2O in the presence of hydrogen, the solution is reduced quickly. 
Copper oxide is disproportionated in the solution of acid and produces copper and copper (II) ions. 

Cupric oxide, when heated with metallic copper, is turned into cuprous oxide. 
In the presence of moisture in the air, oxygen reacts with copper on the surface of any object and cuprous oxide can act as corrosion resistance in such conditions. 
Copper oxide will serve as the protective layer of oxide that is thin. 

Copper oxide is a pure compound of all variations of copper compounds. 
Copper oxide is noticeable because of usability and versatility in physical property. 

Superconductivity at the higher temperature, effects of electron correlations, and spin dynamics make the copper oxide to be useful in many ways. 
Also, both properties, i.e. chemical and physical, are very stable and hence can be easily mixed with water solutions or polymers. 
Furthermore, copper oxide is not expensive. 

The oxide Cu2O that occurs naturally as cuprite and is obtained as red or yellow crystals or powder by oxidation of copper in a furnace or by electrolysis and that is used chiefly as a pigment (as in ceramics and in antifouling paints) and as a seed disinfectant and fungicide.
The monoxide CuO that occurs naturally as paramelaconite and tenorite, is obtained usually in black amorphous form by oxidizing copper, and is used chiefly in preparing cuprammonium solution, as a pigment in ceramics, as a catalyst for hydrogenations, and in chemical analysis.

Physical Properties of Copper Oxide
The Colour of copper oxide is a bit confusing as sometimes you might have seen red or black coloured copper oxides. 
Well, here you should have a clear idea that there are two types of copper oxides like copper(I) oxide that is black in colour and copper (II) oxide that is red. 

Chemical Properties of Copper Oxide:
Copper(I) oxide reacts with water in the presence of oxygen, forms copper(II) hydroxide. 
The chemical equation is given below.
2Cu2O + 4H2O + O2 → 4Cu(OH)2

Copper(I) oxide reacts with hydrogen chloride forms Copper(I) chloride and water. 
The chemical equation is given below.
Cu2O + 2HCl → 2CuCl + H2O

Copper (I) Oxide can react with water as the oxygen is present in the water and make Copper (II) Hydroxide. 

Following is the chemical equation to understand the chemical reaction of copper (I) oxide and water. 
2Cu2O + 4H2O + O2 → 4Cu(OH)2

Through the chemical reaction between hydrogen chloride and copper (I) oxide, Copper (I) Chloride is formed. 
Well, Oxygen of Copper(I) Oxide is reduced with chlorine atoms and form the copper chloride relatively. 

You can understand the chemical reaction between hydrogen chloride and Cu2O from the below chemical equation. 
Cu2O + 2HCl → 2CuCl + H2O

Uses of Copper oxide:
The ship's bottom usually gets affected by seawater, and Copper oxide is essential to cover the bottom with paint and copper oxide is the best option for antifouling paints. 
Copper oxide has the property to control corrosion effectively. 

Copper oxide is a portion of porcelain paints.
Photocells for fabricating rectifiers and light meters contain p-type semiconductors that can be carbon oxide. 

Copper oxide can be used as seed dressing and fungicide. 
They are used in high-tech superconductors, semiconductors and solar-energy transformation. 
Can be implemented in thermoelectric materials, catalyst, superconducting materials, glass, sensing materials, ceramics and other fields. 

Used in antifouling paints for boat and ship bottoms; Copper oxide is an effective control over corrosion.
Used in paints for glass and porcelain.

Used as a p-type semiconductor material that was used to make photocells for light meters and fabricate rectifiers.
Used as a fungicide and seed dressing.

Used as a pigment (glass, ceramics, enamels, glazes, and artificial gems), flux (copper metallurgy, glass fibers, and bronze welding), polishing agent for optical glass, pesticide (antifouling paints, wood preservative, and potato plant and seedling insecticide), solvent for chromic iron ores, and reagent in analytical chemistry.
Also used to make rayon, other copper compounds, acrylates, batteries, electrodes, and magnetic storage devices, for desulfurizing oils, in sweetening petroleum gases, electroplating, purification of hydrogen and waste gases, pyrotechnics, phosphor exciters, catalysts, cloud seeding agents, solar energy devices, cigarette additives, animal feeds, and catalytic converters

Found as the as the mineral tenorite (pure form is a p-type semiconductor)
Other uses include correcting copper deficiencies in soil, in high temperature superconductors, as source of oxygen, in the determination of nitrogen, and as a dietary supplement
Copper I oxide slowly oxidizes in moist air to Copper II oxide.

Industrial Processes with risk of exposure:
Welding
Electroplating
Petroleum Production and Refining
Semiconductor Manufacturing
Battery Manufacturing
Textiles (Fiber & Fabric Manufacturing)
Painting (Pigments, Binders, and Biocides)
Applying Wood Preservatives
Farming (Pesticides)
Glass Manufacturing
Metal Extraction and Refining
Farming (Feed Additives)

Activities with risk of exposure:
Ceramics making 
Enameling

As pigment in glass, ceramics, enamels, porcelain glazes, artificial gems
In mfr of rayon, other copper cmpd
In sweetening petroleum gases
In galvanic electrodes
As flux in copper metallurgy
As optical glass polishing agent
Welding fluxes for bronze
To impart flux and abrasion resistance to glass fibers
In antifouling paints, pyrotechnic compositions
As exciter in phosphor mixtures
As catalyst for org reactions

Used as a heat collecting surface in solar energy devices,
Reduces tar in tobacco smoke,

Used as a catalyst in ammonia manufacture,
For the oxidation of exhaust gases from internal combustion engines uses.

Wood preservation,
Feed additive, 
Pigment, 
Catalyst.

Industry Uses of Copper oxide:
Addition to steel making
Adsorbents and absorbents
Agricultural chemicals (non-pesticidal)
Architectural and electrical products
Catalyst
Elemental metal used in formulation of finished product
Intermediates
Laboratory chemicals
Metal alloy
Metal ingots
Oil and Gas Exploration
Oxidizing/reducing agents
Pigments
Plating agents and surface treating agents
Process regulators
Processing aids, not otherwise listed
Processing aids, specific to petroleum production
Propellants and blowing agents
Smelter feedstock production
copper oxide from baghouse sent for recycling
other industrial function

Consumer Uses of Copper oxide:
Agricultural products (non-pesticidal)
Air care products
Building/construction materials not covered elsewhere
Catalyst
Electrical and electronic products
Explosive materials
Fuels and related products
Metal products not covered elsewhere
Misc. Glass Production
Non-TSCA use
Oil and Gas Exploration
Paints and coatings

Methods of Manufacturing of Copper oxide:
Ignition of copper carbonate or copper nitrate,
Copper oxide can be prepared by oxidation of copper turnings at 800 °c in air or oxygen.
Copper(II) hydroxide is easily converted to the oxide by heating.

General Manufacturing Information of Copper oxide:

Industry Processing Sectors:
Air Purification Absorbent
All other basic inorganic chemical manufacturing
All other basic organic chemical manufacturing
All other chemical product and preparation manufacturing
Asphalt paving, roofing, and coating materials manufacturing
Breathing Air Filtration
Computer and electronic product manufacturing
Construction
Electrical equipment, appliance, and component manufacturing
Explosives manufacturing
Industrial gas manufacturing
Laboratory Use
Mining (except oil and gas) and support activities
Miscellaneous manufacturing
Nonmetallic mineral product manufacturing (includes clay, glass, cement, concrete, lime, gypsum, and other nonmetallic mineral product manufacturing.
Oil and gas drilling, extraction, and support activities
Other - Secondary Precious Metals Reclaimers
Pesticide, fertilizer, and other agricultural chemical manufacturing
Petrochemical manufacturing
Petroleum refineries
Pharmaceutical and medicine manufacturing
Plastic material and resin manufacturing
Primary metal manufacturing
Synthetic dye and pigment manufacturing
Transportation equipment manufacturing
Utilities
Breathing air

Pharmacology and Biochemistry of Copper oxide:

MeSH Pharmacological Classification:

Trace Elements:
A group of chemical elements that are needed in minute quantities for the proper growth, development, and physiology of an organism.

Accidental Release Measures of Copper oxide:

Disposal Methods of Copper oxide:
At the time of review, criteria for land treatment or burial (sanitary landfill) disposal practices are subject to significant revision. 
Prior to implementing land disposal of waste residue (including waste sludge), consult with environmental regulatory agencies for guidance on acceptable disposal practices.

Group III Containers (both combustible and non-combustible) that previously held organic mercury, lead, cadmium, arsenic, or inorganic pesticides should be triple rinsed, punctured and disposed of in a sanitary landfill. 
Non-rinsed containers should be encapsulated and buried at a specially designated landfill site. 

Do not contaminate water by disposal of wastes near a body of water.

Preventive Measures of Copper oxide:
Local exhaust ventilation should be applied wherever there is an incidence of point source emissions or dispersion of regulated contaminants in the work area. 
Ventilation control of the contaminant as close to Copper oxide point of generation is both the most economical and safest method to minimize personnel exposure to airborne contaminants.

The worker should immediately wash the skin when Copper oxide becomes contaminated.
Work clothing that becomes wet or significantly contaminated should be removed and replaced.
The worker should wash daily at the end of each work shift.

Emergency Guidelines of Copper oxide:
FLAMMABLE LIQUIDS-TOXIC/ Health: TOXIC; may be fatal if inhaled, ingested or absorbed through skin. 
Inhalation or contact with some of these materials will irritate or burn skin and eyes. 

Fire will produce irritating, corrosive and/or toxic gases.
Vapors may cause dizziness or suffocation. 
Runoff from fire control or dilution water may cause pollution. 

FLAMMABLE LIQUIDS-TOXIC/ Fire or Explosion: HIGHLY FLAMMABLE: Will be easily ignited by heat, sparks or flames. 
Vapors may form explosive mixtures with air. 
Vapors may travel to source of ignition and flash back. 

Most vapors are heavier than air. 
They will spread along ground and collect in low or confined areas (sewers, basements, tanks). 

Vapor explosion and poison hazard indoors, outdoors or in sewers. 
Those substances designated with a "P" may polymerize explosively when heated or involved in a fire. 

Runoff to sewer may create fire or explosion hazard. 
Containers may explode when heated. 
Many liquids are lighter than water. 

FLAMMABLE LIQUIDS-TOXIC/ Public Safety: CALL Emergency Response Telephone Number.
As an immediate precautionary measure, isolate spill or leak area for at least 50 meters (150 feet) in all directions. 

Keep unauthorized personnel away. 
Stay upwind. 

Keep out of low areas. 
Ventilate closed spaces before entering.

FLAMMABLE LIQUIDS-TOXIC/ Protective Clothing: Wear positive pressure self-contained breathing apparatus (SCBA). 
Wear chemical protective clothing that is specifically recommended by the manufacturer. 

Copper oxide may provide little or no thermal protection. 
Structural firefighters' protective clothing provides limited protection in fire situations ONLY; it is not effective in spill situations where direct contact with the substance is possible.

Information of Copper oxide:
CAS number: 1317-38-0
EC number: 215-269-1
Grade: ACS
Hill Formula: CuO
Molar Mass: 79.54 g/mol
HS Code: 2825 50 00
Quality Level: MQ100

Physicochemical Information of Copper oxide:
Density: 6.32 g/cm3
Melting Point: 1336 °C
Bulk density: 2200 kg/m3

Properties of Copper oxide:
Molecular Weight: 79.55
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 1
Rotatable Bond Count: 0
Exact Mass: 78.924512
Monoisotopic Mass: 78.924512
Topological Polar Surface Area: 17.1 Ų
Heavy Atom Count    : 2
Complexity: 2
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 1
Compound Is Canonicalized: Yes

Specifications of Copper oxide:
Assay (oxygen demand as CuO):m≥ 55.0 %
Chloride (Cl): ≤ 0.005 %
Total carbon (C): ≤ 0.002 %
Total nitrogen (N):m≤ 0.002 %
Total sulfur (as SO₄): ≤ 0.005 %

Synonyms of Copper oxide:
Copper(II) oxide
CUPRIC OXIDE
Copper oxide
1317-38-0
oxocopper
Copper oxide (CuO)
Copper monoxide
Black copper oxide
Banacobru ol
Chrome Brown
Copper Brown
Copper monooxide
Copper(2+) oxide
C.I. Pigment Black 15
Copper (II) oxide
Cu-O Linkage
C.I. 77403
MFCD00010979
CuO
Paramelaconite
Copacaps
Copporal
Natural tenorite
Wolmanac concentrate
Boliden Salt K-33
Caswell No. 265
CI Pigment black 15
Boliden-CCA Wood Preservative
CCA Type C Wood Preservative
HSDB 266
Osmose K-33 Wood Preservative
Osmose P-50 Wood Preservative
Osmose K-33-A Wood Preservative
Osmose K-33-C Wood Preservative
EINECS 215-269-1
NSC 83537
EPA Pesticide Chemical Code 042401
CI 77403
copper-oxygen
Farboil Super Tropical Anti-Fouling 1260
copper(II)oxide
Copper Oxide Ink
Copper oxide, CuO
Copper Oxide Powder
copper-(II) oxide
Copper Oxide Dispersion
Copper Oxide Nanopowder
Cupric Oxide Nanopowder
Copper oxide nano-chains
Copper(II) oxide, CP
Copper Oxide Nanoparticles
Copper(II) oxide, powder
EC 215-269-1
Copper(II) oxide, Puratronic?
DTXSID5034488
Copper Oxide Powder, 99+% Nano
NSC83537
Copper(II) oxide, LR, >=97%
Copper Oxide Nanoparticles Dispersion
NSC-83537
AKOS015950660
Copper(II) oxide (99.995%-Cu)
Copper Oxide Nanoparticles / Nanopowder
Copper(II) oxide, ACS reagent, >=99.0%
Copper(II) oxide, powder, <10 mum, 98%
CS-0016015
FT-0624050
Y1305
Chromium Silicide (CrSi2) Sputtering Targets
Copper(II) oxide, >=99.0% (RT), granular
Copper(II) oxide, 99.999% trace metals basis
Copper(II) oxide, p.a., ACS reagent, 99.0%
J-520121
Q27458610
Copper(II) oxide, powder, 99.99% trace metals basis
Copper(II) oxide, powder, 99.995% trace metals basis
Copper(II) oxide, nanopowder, <50 nm particle size (TEM)
Copper(II) oxide, puriss. p.a., >=99.0% (RT), powder
Copper(II) oxide, nanotubes, diam. x L 10-12 nm x 75-100 nm
Copper(II) oxide, needles, mixture of CuO and Cu2O, ACS reagent
PEDOT PSS Poly(3,4-ethylenedioxythiophene)-poly(styrenesulfonate )
Copper(II) oxide on alumina, 14-20 mesh, extent of labeling: 13 wt. % loading