- Sodium cyanide
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Sodium cyanide Identifiers CAS number 143-33-9 
PubChem 8929 ChemSpider 8587 UN number 1689 ChEMBL CHEMBL1644697 
RTECS number VZ7525000 Jmol-3D images Image 1 - [C-]#N.[Na+]
- InChI=1S/CN.Na/c1-2;/q-1;+1
Key: MNWBNISUBARLIT-UHFFFAOYSA-N
InChI=1/CN.Na/c1-2;/q-1;+1
Key: MNWBNISUBARLIT-UHFFFAOYAG
Properties Molecular formula NaCN Molar mass 49.0072 g/mol Appearance white solid Density 1.595 g/cm3 Melting point 563.7 °C
Boiling point 1496 °C
Solubility in water 58 g/100 ml (20 °C) (hydrate solubility), 82 g/100 ml (34.7 °C) Refractive index (nD) 1.45 Hazards MSDS ICSC 1118 EU Index 006-007-00-5 EU classification Very toxic (T+)
Dangerous for the environment (N)Corrosive (C) [1]R-phrases R26/27/28, R32, R50/53 S-phrases (S1/2), S7, S28, S29, S45, S60, S61 NFPA 704 
030Flash point Non-flammable LD50 5.8–15 mg/kg (oral in rats, mice)[2] Related compounds Other cations Potassium cyanide Related compounds Hydrogen cyanide 
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Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)Infobox references Sodium cyanide is an inorganic compound with the formula NaCN. This highly toxic colorless salt is used mainly in gold mining but has other niche applications. It is an inorganic salt derived from neutralization reactions involving the weak acid hydrogen cyanide.
Contents
Production and chemical properties
Sodium cyanide is produced by treating hydrogen cyanide with sodium hydroxide:[3]
- HCN + NaOH → NaCN + H2O
Worldwide production was estimated at 500,000 tons in the year 2006. In former times, it was prepared by the Castner-Kellner process involving the reaction of sodium amide with carbon at elevated temperatures.
- NaNH2 + C → NaCN + H2
The structure of solid NaCN is related to that of sodium chloride.[4] The anions and cations are each six-coordinate (potassium chloride (KCN) has a similar structure). Each Na+ forms pi-bonds to two CN- groups as well as two "bent" Na---CN and two "bent" Na---NC links.[5]
Because the salt is derived from a weak acid, NaCN readily reverts back to HCN by hydrolysis: the moist solid emits small amounts of hydrogen cyanide, which smells like bitter almonds (not everyone can smell it—the ability thereof is due to a genetic trait[6]). Sodium cyanide reacts rapidly with strong acids to release hydrogen cyanide. This dangerous process represents a significant risk associated with cyanide salts. It is detoxified most efficiently with hydrogen peroxide (H2O2) to produce sodium cyanate (NaOCN) and water:[3]
- NaCN + H2O2 → NaOCN + H2O
Applications
Cyanide mining
Further information: cyanide processSodium gold cyanide
Sodium cyanide is mainly used to extract gold and other precious metals in mining. This application exploits the high affinity of gold(I) for cyanide, which induces gold metal to oxidize and dissolve in the presence of air and water, producing the salt sodium gold cyanide (or gold sodium cyanide) and sodium hydroxide:
- 4 Au + 8 NaCN + O2 + 2 H2O → 4 Na[Au(CN)2] + 4 NaOH
A similar process uses potassium cyanide (KCN, a close relative of sodium cyanide) to produce potassium gold cyanide (KAu(CN2)).
Few other methods exist for this extraction process.
Chemical feedstock
Several commercially significant chemical compounds are derived from cyanide, including cyanuric chloride, cyanogen chloride, and many nitriles. In organic synthesis, cyanide, which is classified as a strong nucleophile, is used to prepare nitriles, which occur widely in many specialty chemicals, including pharmaceuticals.
Niche uses
Being highly toxic, sodium cyanide is used to kill or stun rapidly such as in illegal cyanide fishing and in collecting jars used by entomologists.
Toxicity
Main article: Cyanide poisoningCyanide salts are among the most rapidly acting of all known poisons. Cyanide is a potent inhibitor of respiration, acting on mitochondrial cytochrome oxidase and hence blocking electron transport. This results in decreased oxidative metabolism and oxygen utilization. Lactic acidosis then occurs as a consequence of anaerobic metabolism.
References
- ^ Oxford MSDS
- ^ Martel, B.; Cassidy, K. (2004). Chemical Risk Analysis: A Practical Handbook. Butterworth–Heinemann. pp. 361. ISBN 1903996651.
- ^ a b Andreas Rubo, Raf Kellens, Jay Reddy, Norbert Steier, Wolfgang Hasenpusch "Alkali Metal Cyanides" in Ullmann's Encyclopedia of Industrial Chemistry 2006 Wiley-VCH, Weinheim, Germany. doi:10.1002/14356007.i01_i01
- ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
- ^ H. T. Stokes, D. L. Decker, H. M. Nelson, J. D. Jorgensen (1993). "Structure of potassium cyanide at low temperature and high pressure determined by neutron diffraction". Phys. Rev. B 47 (17): 11082–11092. doi:10.1103/PhysRevB.47.11082.
- ^ Online 'Mendelian Inheritance in Man' (OMIM) 304300
See also
External links
- Institut national de recherche et de sécurité (1997). "Cyanure de sodium. Cyanure de potassium". Fiche toxicologique n° 111, Paris:INRS, 6pp. (PDF file, in French)
- International Chemical Safety Card 1118
- Hydrogen cyanide and cyanides (CICAD 61)
- National Pollutant Inventory - Cyanide compounds fact sheet
- NIOSH Pocket Guide to Chemical Hazards
- EINECS number 205-599-4
- CID 8929 from PubChem
- CSST (Canada)
- Sodium cyanide hazards to fish and other wildlife from gold
Sodium compounds NaAlO2 · NaBH3(CN) · NaBH4 · NaBr · NaBrO3 · NaCH3COO · NaCN · NaC6H5CO2 · NaC6H4(OH)CO2 · NaCl · NaClO · NaClO2 · NaClO3 · NaClO4 · NaF · NaH · NaHCO3 · NaHSO3 · NaHSO4 · NaI · NaIO3 · NaIO4 · NaMnO4 · NaNH2 · NaNO2 · NaNO3 · NaN3 · NaOH · NaO2 · NaPO2H2 · NaReO4 · NaSCN · NaSH · NaTcO4 · NaVO3 · Na2CO3 · Na2C2O4 · Na2CrO4 · Na2Cr2O7 · Na2MnO4 · Na2MoO4 · Na2O · Na2O2 · Na2O(UO3)2 · Na2S · Na2SO3 · Na2SO4 · Na2S2O3 · Na2S2O4 · Na2S2O5 · Na2S2O6 · Na2S2O7 · Na2S2O8 · Na2Se · Na2SeO3 · Na2SeO4 · Na2SiO3 · Na2Te · Na2TeO3 · Na2Ti3O7 · Na2U2O7 · NaWO4 · Na2Zn(OH)4 · Na3N · Na3P · Na3VO4 · Na4Fe(CN)6 · Na5P3O10 · NaBiO3
Categories:- Cyanides
- Sodium compounds
- Photographic chemicals
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