09-07-2021-1333 - cyanogen (CN)2 1815 prussia

 Cyanogen is the chemical compound with the formula (CN)₂. It is a colorless, toxic gas with a pungent odor. The molecule is a pseudohalogen. Cyanogen molecules consist of two CN groups – analogous to diatomic halogen molecules, such as Cl₂, but far less oxidizing. The two cyano groups are bonded together at their carbon atoms: N≡C−C≡N, although other isomers have been detected.^[6] The name is also used for the CN radical,^[7] and hence is used for compounds such as cyanogen bromide (NCBr).^[8]

Cyanogen is the anhydride of oxamide:

H₂NC(O)C(O)NH₂ → NCCN + 2 H₂O

although oxamide is manufactured from cyanogen by hydrolysis:^[9]

NCCN + 2 H₂O → H₂NC(O)C(O)NH₂

NamesPreferred IUPAC name

Oxalonitrile^[4]

Systematic IUPAC name

Ethanedinitrile^[4]

Other names

Cyanogen
Bis(nitridocarbon)(C—C)^[1]
Dicyan^[2][3]
Carbon nitride^[2]
Oxalic acid dinitrile^[3]
Dicyanogen
Nitriloacetonitrile

Identifiers

CAS Number

• 460-19-5 
  3D model (JSmol)
  • Interactive image
  Beilstein Reference
  1732464ChEBI
  • CHEBI:29308 ChemSpider
    • 9605 ECHA InfoCard100.006.643 EC Number
      • 207-306-5
      Gmelin Reference
      1090MeSHcyanogen
      PubChem CID
      • 9999
      RTECS number
      • GT1925000
      UNII
      • 534Q0F66RK UN number1026
        CompTox Dashboard (EPA)
        • DTXSID1023992 
        show

        InChI
        show

        SMILES
        Properties
        Chemical formula
        (CN)₂Molar mass52.034 g/mol AppearanceColourless gasOdorpungent, almond-likeDensity950 mg mL⁻¹ (at −21 °C)Melting point−28 °C (−18 °F; 245 K) Boiling point−21.1 °C; −6.1 °F; 252.0 K 
        Solubility in water
        45 g/100 mL (at 20 °C)Solubilitysoluble in ethanol, ethyl etherVapor pressure5.1 atm (21 °C)^[5]
        Henry's law
        constant (k_H)
        1.9 μmol Pa⁻¹ kg⁻¹
        Magnetic susceptibility (χ)
        -21.6·10⁻⁶ cm³/mol
        Refractive index(n_D)
        1.327 (18 °C)Thermochemistry
        Std molar
        entropy (S^o₂₉₈)
        241.57 J K⁻¹ mol⁻¹
        Std enthalpy of
        formation(Δ_fH^⦵₂₉₈)
        309.07 kJ mol⁻¹
        Std enthalpy of
        combustion(Δ_cH^⦵₂₉₈)
        −1.0978–−1.0942 MJ mol⁻¹HazardsMain hazardsforms cyanide in the body; flammable^[5]Safety data sheetinchem.orgGHS pictogramsGHS Signal wordDanger
        GHS hazard statements
        H220, H331, H400, H410
        GHS precautionary statements
        P210, P261, P271, P273, P304+340, P311, P321, P377, P381, P391, P403, P403+233, P405, P501NFPA 704(fire diamond)
        

        4

        4

        2
        Explosive limits6.6–32%^[5]NIOSH (US health exposure limits):
        PEL(Permissible)
        none^[5]
        REL(Recommended)
        TWA 10 ppm (20 mg/m³)^[5]
        IDLH (Immediate danger)
        N.D.^[5]Related compounds
        Related alkanenitriles
        • Hydrogen cyanide
        • Thiocyanic acid
        • Cyanogen iodide
        • Cyanogen bromide
        • Cyanogen chloride
        • Cyanogen fluoride
        • Cyanogen azide
        • Acetonitrile
        • Aminoacetonitrile
        • Glycolonitrile
        • Propionitrile
        • Aminopropionitrile
        • Malononitrile
        • Pivalonitrile
        • Acetone cyanohydrin
        Related compounds
        DBNPA

_{https://en.wikipedia.org/wiki/Cyanogen}

_{Cyanogen produces the second-hottest-known natural flame (after carbon subnitride) with a temperature of over 4,525 °C (8,177 °F) when it burns in oxygen.^[20][21]}

Cyanogen was first synthesized in 1815 by Joseph Louis Gay-Lussac, who determined its empirical formula and named it. Gay-Lussac coined the word "cyanogène" from the Greek words κυανός (kyanos, blue) and γεννάω (gennao, I create), because cyanide was first isolated by the Swedish chemist Carl Wilhelm Scheele from the pigment "Prussian blue".^[14] By the 1850s, cyanogen soap was used by photographers to remove silver stains from their hands.^[15] It attained importance with the growth of the fertilizer industry in the late 19th century and remains an important intermediate in the production of many fertilizers. 

It is also used as a stabilizer in the production of nitrocellulose.

In 1910 a spectroscopic analysis of Halley's Comet found cyanogen in the comet's tail, which led to public fear that the Earth would be poisoned as it passed through the tail. Because of the extremely diffuse nature of the tail, there was no effect when the planet passed through it.^[16][17]

https://en.wikipedia.org/wiki/Cyanogen