Physical Properties Occurrence Uses Preparation Reactions
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Nickel(II) oxide

Physical Properties Occurrence Uses Preparation Reactions
Nickel(II) oxide Structure
Nickel(II) oxide
  • CAS No.1313-99-1
  • Chemical Name:Nickel(II) oxide
  • CBNumber:CB2358284
  • Molecular Formula:NiO
  • Formula Weight:74.69
  • MOL File:1313-99-1.mol
Nickel(II) oxide Property
  • Melting point: :1960 °C
  • Density  :6.67 g/mL at 25 °C(lit.)
  • form  :Powder/Solid
  • color  :green
  • Specific Gravity :6.67
  • Water Solubility  :insoluble
  • Merck  :14,6512
  • Stability: :Stable. Incompatible with strong acids.
  • InChIKey :GNRSAWUEBMWBQH-UHFFFAOYSA-N
  • CAS DataBase Reference :1313-99-1(CAS DataBase Reference)
  • EWG's Food Scores :5
  • EPA Substance Registry System :Nickel(II) oxide (1313-99-1)
Safety
Hazard and Precautionary Statements (GHS)
  • Symbol(GHS)
  • Signal wordDanger
  • Hazard statements H350-H317-H350i-H372-H413
  • Precautionary statements P201-P280-P308+P313-P260-P405-P501a
Nickel(II) oxide Price More Price(28)
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  • Product number: 203882
  • Product name : Nickel(II) oxide
  • Purity: 99.99% trace metals basis
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  • Product number: 203882
  • Product name : Nickel(II) oxide
  • Purity: 99.99% trace metals basis
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  • Product name : Nickel(II) oxide, Puratronic?, 99.998% (metals basis)
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  • Product name : Nickel(II) oxide, Puratronic?, 99.998% (metals basis)
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Nickel(II) oxide Chemical Properties,Usage,Production

  • Physical Properties Green cubic crystals; transforms to a grayish black octahedral form, known as black oxide, when strongly ignited; black oxide has a metallic luster; density of green oxide is 6.72 g/cm3; Mohs hardness 5.5; melts at 1955°C; insoluble in water; soluble in acids at ordinary temperatures; black form dissolves in hot acids.
    Nickel (II) oxide
  • Occurrence The oxide occurs in nature in the mineral, bunsenite.
  • Uses Nickel (II) oxide is used in the ceramic industry for making frit, ferrites, and coloring porcelain. The oxide in sinter form is used in the production of nickel- steel alloys. It supplies oxygen to the melt for removal of carbon as carbon dioxide. Some other important uses of Nickel (II) oxide include preparation of many nickel salts, specialty chemicals, and nickel catalysts. It also is used as an electrode in fuel cells.
  • Preparation Nickel (II) oxide is prepared by heating pure nickel powder with oxygen at a temperature above 400°C. In some commercial processes, green Nickel (II) oxide is made by heating a mixture of nickel powder and water in air at 1,000°C. Adding some Nickel (II) oxide to the above mixture enhances the rate of reaction. An alternative method of preparation of the green oxide involves thermal decomposition of an oxo acid salt of nickel at elevated temperatures. Thus, nickel nitrate, nickel sulfate or, more conveniently, nickel carbonate when heated at 1,000°C, yields the green oxide. The black oxide, on the other hand, is produced at a lower temperature from incomplete calcination of the carbonate or nitrate salt at 600°C. The oxygen content of the black form is slightly greater than its green counterpart.
  • Reactions Several nickel salts are obtained by reactions of nickel oxide with mineral acids. Thus, the reaction of black nickel oxide with hot dilute sulfuric acid forms nickel sulfate, NiSO4•6H2O. Similarly, dilute nitric acid, hydrochloric, and hydrobromic acids when heated react with the black form of nickel oxide to yield corresponding nickel salts as hexahydrates.
    Heating nickel oxide with hydrogen, carbon, or carbon monoxide reduces it to metallic nickel.
    Nickel oxide combines with sodium or potassium hydroxide at elevated temperatures (>700°C), forming sodium or potassium nickelate; i.e., K2NiO2:
    NiO + 2NaOH → Na2NiO2 + H2O
  • Chemical Properties Nickel(II) oxide is Brownish black or black powder.
  • Uses Nickel salts, porcelain painting, fuel cell electrodes.
  • Preparation Nickel oxide is prepared by heating pure nickel powder with oxygen at a temperature above 400°C. In some commercial processes, green nickel oxide is made by heating a mixture of nickel powder and water in air at 1,000°C. Adding some nickel oxide to the above mixture enhances the rate of reaction. An alternative method of preparation of the green oxide involves thermal decomposition of an oxo acid salt of nickel at elevated temperatures. Thus, nickel nitrate, nickel sulfate or, more conveniently, nickel carbonate when heated at 1,000°C, yields the green oxide. The black oxide, on the other hand, is produced at a lower temperature from incomplete calcination of the carbonate or nitrate salt at 600°C. The oxygen content of the black form is slight-ly greater than its green counterpart.
  • Reactions Nickel(II) oxide is insoluble in water but soluble in acids as long as it has not been ignited at a high temperature (under these latter conditions it is converted into grey-black octahedra having a metallic lustre). It reacts reversibly with hydrogen, the reaction NiO+H2 ? Ni+H20 proceeding from left to right at relatively low temperatures in a stream of hydrogen.
  • Hazard Confirmed carcinogen.
  • Safety Profile Confirmed carcinogen with experimental carcinogenic and tumorigenic data. Poison by intratracheal, intravenous, and subcutaneous routes. Mutation data reported. Can react violently with fluorine, hydrogen peroxide, hydrogen sulfide, iodine, barium oxide + air. See also NICKEL COMPOUNDS.
Nickel(II) oxide Preparation Products And Raw materials
Raw materials
Preparation Products
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