Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Potassium cyanate: Difference between pages

| Watchedfields = changed

| verifiedrevid = 477000524

| ImageFile = <chem>\mathsf{K+\ \ ^-N=C=O}</chem>

| ImageFile1 = Potassium cyanate.jpg

| ImageFileL1 = Potassium-3D.png

| ImageFileR1 = Cyanate-ion-3D-vdW.png

| ImageSize =

| IUPACName = Potassium cyanate

| OtherNames =

| Section1 = {{Chembox Identifiers

| CASNo_Ref = {{cascite|correct|CAS}}

| CASNo = 590-28-3

| Beilstein = 3560091

| ChEBI_Ref = {{ebicite|correct|EBI}}

| ChEBI = 38904

| ChEMBL = 4079232

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| EINECS = 209-676-3

| Gmelin = 21361

| PubChem = 11378442

| RTECS = GS6825000

| KEGG_Ref = {{keggcite|correct|kegg}}

| KEGG = C19067

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = G9C31TWN5M

| Section2 = {{Chembox Properties

| Formula = KOCN

| MolarMass = 81.1151 g/mol

| Appearance = white, crystalline powder

| Density = 2.056 g/cm³

| = 315

| BoilingPt= ~

| BoilingPtC = 700

| BoilingPt_notes = decomposes

| Solubility = 75 g/100 mL

| SolubleOther = very slightly soluble in alcohol

| Section3 = {{Chembox Structure

| CrystalStruct = tetragonal

}}

| Section7 = {{Chembox Hazards

| MainHazards =

| NFPA-H = 2

| NFPA-F = 0

| NFPA-R = 0

| NFPA-S =

| GHSPictograms = {{GHS07}}

| GHSSignalWord = Warning

| HPhrases = {{H-phrases|302}}

| PPhrases = {{P-phrases|264|270|301+312|330|501}}

| LD50 = 841 mg/kg (oral, rat)

| FlashPt =

| AutoignitionPt =

}}

'''Potassium cyanate''' is an [[inorganic compound]] with the [[chemical formula|formula]] KOCN (sometimes denoted KCNO<ref>Recreation of Wöhler’s Synthesis of Urea: An Undergraduate Organic Laboratory Exercise'' James D. Batchelor, Everett E. Carpenter, Grant N. Holder, Cassandra T. Eagle, Jon Fielder, Jared Cummings The Chemical Educator 1/Vol .3,NO.6 '''1998''' ISSN 1430-4171 [http://chemeducator.org/sbibs/s0003006/spapers/36eag897.pdf Online article] {{webarchive|url=https://web.archive.org/web/20060930231240/http://chemeducator.org/sbibs/s0003006/spapers/36eag897.pdf |date=2006-09-30 }}</ref>). It is a colourless solid. It is used to prepare many other compounds including useful [[herbicide]]. Worldwide production of the potassium and sodium salts was 20,000 tons in 2006.<ref name=Ullmann>Peter M. Schalke1, "Cyanates, Inorganic Salts" Ullmann's Encyclopedia of Industrial Chemistry2006, Wiley-VCH, Weinheim. {{doi|10.1002/14356007.a08_157.pub2}}. Article Online Posting Date: July 15, 2006</ref>

==Structure and bonding==

The [[cyanate]] [[anion]] is isoelectronic with [[carbon dioxide]] and with the [[azide]] anion, being linear. The C-N distance is 121&nbsp;pm, about 5&nbsp;pm longer than for [[cyanide]].<ref>{{Greenwood&Earnshaw2nd}}</ref><ref>Jursík, F. (2001). Anorganická chemie nekovů (1. vydání). VŠCHT Praha. {{ISBN|80-7080-417-3}}</ref> Potassium cyanate is isostructural with [[potassium azide]].<ref>T. C. Waddington "Lattice parameters and infrared spectra of some inorganic cyanates" J. Chem. Soc., 1959, 2499-2502. {{doi|10.1039/JR9590002499}}</ref>

[[File:KN3viewCropped.tif|thumb|left|220px|Structure of [[potassium azide]],<ref>Ulrich Müller "Verfeinerung der Kristallstrukturen von KN3, RbN3, CsN3 und TIN3" Zeitschrift für anorganische und allgemeine Chemie 1972, Volume 392, 159–166. {{doi|10.1002/zaac.19723920207}}</ref> which is isostructural with potassium cyanate.]]

==Uses==

The potassium and sodium salts can be used interchangeably for the majority of applications. Potassium cyanate is often preferred to the sodium salt, which is less soluble in water and less readily available in pure form.

Potassium cyanate is used as a basic raw material for various organic syntheses, including, [[urea]] derivatives, [[semicarbazide]]s, [[carbamate]]s and [[isocyanate]]s. For example, it is used to prepare the drug [[Hydroxycarbamide|hydroxyurea]]. It is also used for the [[heat treatment]] of metals (e.g., [[Ferritic nitrocarburizing]]).<ref name=Ullmann/><ref>INEOS Paraform GmbH, ''Potassium Cyanate (KOCN) product information.'' [http://www.ineosparaform.com/files/potassium_cyanate_english.pdf Online version] accessed on 2009-06-30.</ref>

===Therapeutic uses===

Potassium cyanate has been used to reduce the percentage of sickled erythrocytes under certain conditions and has also increased the number of deformalities. In an aqueous solution, it has prevented irreversibly the in vitro sickling of hemoglobins containing human erythrocytes during deoxygenization. Veterinarians have also found potassium cyanate useful in that the cyanate salts and isocyanates can treat parasite diseases in both birds and mammals.<ref>[https://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=11378442&loc=ec_rcs. "Potassium Cyanate"]</ref>

==Preparation and reactions==

KOCN is prepared by heating [[urea]] with [[potassium carbonate]] at 400&nbsp;°C:

:2 OC(NH₂)₂ + K₂CO₃ → 2 KOCN + (NH₄)₂CO₃

The reaction produces a liquid. Intermediates and impurities include [[biuret]], [[cyanuric acid]], and potassium allophanate (KO₂CNHC(O)NH₂), as well as unreacted starting urea, but these species are unstable at 400&nbsp;°C.<ref name=Ullmann/>

Protonation gives a 97:3 mixture (at room temperature) of two [[tautomer]]s, HNCO ([[isocyanic acid]]) and NCOH (cyanic acid). This mixture is stable at high dilution but trimerizes on concentration to give [[cyanuric acid]].

==Properties==

Potassium carbonate crystals are destroyed by the melting process so that the urea can react with almost all potassium ions to convert to potassium cyanate at a higher rate than when in the form of a salt. This makes it easier to reach higher purities above 95%. It can also be made by oxidizing potassium cyanide at a high temperature in the presence of oxygen or easily reduced oxides, such as lead, tin, or manganese dioxide, and in aqueous solution by reacting with hypochlorites or hydrogen peroxide. Another way to synthesize it is to allow an alkali metal cyanide to react with oxygen in nickel containers under controlled conditions. It can be formed by the oxidation of ferrocyanide. Lastly, it can be made by heating potassium cyanide with lead oxide.<ref>"Potassium cyanate" https://pubchem.ncbi.nlm.nih.gov/summary/summary.cgi?cid=11378442&loc=ec_rcs</ref>

==References==

{{reflist}}

== External links ==

* [https://web.archive.org/web/20060718001129/http://www.catalogue.fisher.co.uk/scripts/search.dll?ViewMSDS&SheetNumber=88624 MSDS]

* [http://hazard.com/msds/mf/baker/baker/files/p5697.htm MSDS at jtbaker.com]

{{Potassium compounds}}

{{Cyanates}}

[[Category:Potassium compounds]]

[[Category:Cyanates]]