Sodium cyanide

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Sodium cyanide
Sodium cyanide bonding
Sodium-cyanide-phase-I-unit-cell-3D-SF.png
Identifiers
  • 143-33-9 checkY
3D model (JSmol)
ChEMBL
ChemSpider
ECHA InfoCard 100.005.091 Edit this at Wikidata
EC Number
  • 205-599-4
RTECS number
  • VZ7525000
UNII
UN number 1689
Properties
Chemical formula
 NaCN
Molar mass 49.0072 g/mol
Appearance white solid
Odor faint almond-like
Density 1.5955 g/cm3
Melting point 563.7 °C (1,046.7 °F; 836.9 K)
Boiling point 1,496 °C (2,725 °F; 1,769 K)
48.15 g/100 mL (10 °C)
63.7 g/100 mL (25 °C)
Solubility soluble in ammonia, methanol, ethanol
very slightly soluble in dimethylformamide, SO2
insoluble in dimethyl sulfoxide
Refractive index (nD)
 1.452
Thermochemistry
70.4 J/mol K
115.7 J/mol K
Std enthalpy of
formation (ΔfH⦵298)
 -91 kJ/mol
Hazards
Safety data sheet ICSC 1118
GHS pictograms GHS06: Toxic GHS09: Environmental hazard
NFPA 704 (fire diamond)
4
0
0
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)
 6.44 mg/kg (rat, oral)
4 mg/kg (sheep, oral)
15 mg/kg (mammal, oral)
8 mg/kg (rat, oral)[2]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 5 mg/m3[1]
REL (Recommended)
 C 5 mg/m3 (4.7 ppm) [10-minute][1]
IDLH (Immediate danger)
 25 mg/m3 (as CN)[1]
Related compounds
Other cations
 Potassium cyanide
Related compounds
 Hydrogen cyanide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Sodium cyanide is a poisonous compound with the formula NaCN. It is a white, water-soluble solid. Cyanide has a high affinity for metals, which leads to the high toxicity of this salt. Its main application, in gold mining, also exploits its high reactivity toward metals. It is a moderately strong base. When treated with acid, it forms the toxic gas hydrogen cyanide:

NaCN + H2SO4 → HCN + NaHSO4

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. Formerly it was prepared by the Castner 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 cyanide (KCN) adopts 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, sodium cyanide readily reverts to HCN by hydrolysis; the moist solid emits small amounts of hydrogen cyanide, which is thought to smell 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[]

See also: Cyanide process

Sodium gold cyanide[]

Sodium cyanide is used mainly to extract gold and other precious metals in mining industry. This application exploits the high affinity of gold(I) for cyanide, which induces gold metal to oxidize and dissolve in the presence of air (oxygen) 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(CN)2). 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 chemicals, including pharmaceuticals. Illustrative is the synthesis of benzyl cyanide by the reaction of benzyl chloride and sodium cyanide.[7]

Niche uses[]

Being highly toxic, sodium cyanide is used to kill or stun rapidly such as in widely illegal cyanide fishing and in collecting jars used by entomologists.

Homicide[]

In 1986, Stella Nickell murdered her husband Bruce Nickell with sodium cyanide. In order to disguise her being responsible for the murder, she placed several bottles of Excedrin tainted with sodium cyanide on store shelves near her home in Tacoma, WA. Susan Snow, a bank manager living nearby in the same town, died several days later from taking some of the tainted Excedrin.

In 1991, Joseph Meling, a resident of Tumwater, WA, copied Nickell's idea, this time tainting capsules of Sudafed on store shelves near his home to murder his wife and disguise the incident as a mass murder. Meling had forged life insurance in his wife's name totaling $700,000. Meling's wife Jennifer Meling survived the poisoning attempt but two other residents of Tumwater died after taking the tainted Sudafed.

Toxicity[]

Main article: Cyanide poisoning

Sodium cyanide, like other soluble cyanide salts, is among the most rapidly acting of all known poisons. NaCN 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. An oral dosage as small as 200–300 mg can be fatal.

References[]

  1. ^ Jump up to: a b c NIOSH Pocket Guide to Chemical Hazards. "#0562". National Institute for Occupational Safety and Health (NIOSH).
  2. ^ "Cyanides (as CN)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  3. ^ Jump up to: 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
  4. ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
  5. ^ 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 (Submitted manuscript). 47 (17): 11082–11092. doi:10.1103/PhysRevB.47.11082. PMID 10005242.
  6. ^ Online Mendelian Inheritance in Man (OMIM): 304300
  7. ^ Adams, Roger; Thal, A. F. (1922). "Benzyl cyanide". Organic Syntheses. 2: 9. doi:10.15227/orgsyn.002.0009.

External links[]

  • v
  • t
Salts and covalent derivatives of the cyanide ion
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