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The cyanide ion is a reductant and is oxidized by strong oxidizing agents such as molecular chlorine (Cl 2), hypochlorite (ClO −), and hydrogen peroxide (H 2 O 2). These oxidizers are used to destroy cyanides in effluents from gold mining .
Any salt containing the ion, such as ammonium cyanate, is called a cyanate. The cyanate ion is an isomer of the much-less-stable fulminate anion, CNO − or [C − ≡N + −O −]. [1] The cyanate ion is an ambidentate ligand, forming complexes with a metal ion in which either the nitrogen or oxygen atom may be the electron-pair donor.
A CN bond is strongly polarized towards nitrogen (the electronegativities of C and N are 2.55 and 3.04, respectively) and subsequently molecular dipole moments can be high: cyanamide 4.27 D, diazomethane 1.5 D, methyl azide 2.17, pyridine 2.19. For this reason many compounds containing CN bonds are water-soluble.
Cyanogen is typically generated from cyanide compounds. One laboratory method entails thermal decomposition of mercuric cyanide: . 2 Hg(CN) 2 → (CN) 2 + Hg 2 (CN) 2 Or, one can combine solutions of copper(II) salts (such as copper(II) sulfate) with cyanides; an unstable copper(II) cyanide is formed which rapidly decomposes into copper(I) cyanide and cyanogen.
Pentacyanocobaltate ([Co(CN) 5] 3−) is produced by the addition of five or more equivalents of a cyanide to a solution of a cobalt(II) salt. It is square pyramidal. [ 5 ] Solutions of [Co(CN) 5 ] − 3 undergo a variety of reactions, such as hydrogenation: [ 6 ]
The ion has cyanide groups arranged in a square around the central nickel ion. The symmetry of the ion is D 4h. The distance from the nickel atom to the carbon is 1.87 Å, and the carbon-nitrogen distance is 1.16 Å. [1] In their crystals, the tetracyanonickelate(II) anions are often arranged in a columnar structure (e.g. in K 2 [Ni(CN) 4] [2]).
A spectral line of • CN was detected in 1938 in the interstellar medium in the ultraviolet, and was identified in 1940 by Andrew McKellar. The coudé spectrograph and a 100-inch (2.5 m) telescope were used to observe • CN's interstellar lines and ultraviolet spectra. Use of the spectrograph confirmed McKellar's findings and also made the ...
Ferricyanide is the name of the anion [Fe 6] 3−. It is also called hexacyanoferrate(III) and in rare, but systematic nomenclature , hexacyanidoferrate(III). The most common salt of this anion is potassium ferricyanide , a red crystalline material that is used as an oxidant in organic chemistry .