Calcium phosphide

Calcium phosphide
Names
IUPAC name
Calcium phosphide
Other names
Photophor, CP, Polythanol
Identifiers
3D model (JSmol)
ECHA InfoCard 100.013.766
Properties
Ca3P2
Molar mass 182.18 g/mol
Appearance red-brown crystalline powder or grey lumps
Density 2.51 g/cm3
Melting point ~1600 °C
decomposes
Hazards
Main hazards Source of toxic phosphine, dangerous reaction with water
R-phrases (outdated) R15/29 R28 R50
S-phrases (outdated) (S1/2) S22 S43 S45 S61
NFPA 704
Flammability code 0: Will not burn. E.g., waterHealth code 4: Very short exposure could cause death or major residual injury. E.g., VX gasReactivity code 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g., fluorineSpecial hazard W: Reacts with water in an unusual or dangerous manner. E.g., cesium, sodiumNFPA 704 four-colored diamond
0
4
3
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

Calcium phosphide (CP) is the inorganic compound with the formula Ca3P2. It is one of several phosphides of calcium, being described as the salt-like material composed of Ca2+ and P3−. Other, more exotic calcium phosphides have the formula CaP, CaP3, Ca2P2, and Ca5P8.

Ca3P2 has the appearance of red-brown crystalline powder or grey lumps. Its trade name is Photophor for the incendiary use or Polytanol for the use as rodenticide.[1]

Preparation and structure

It may be formed by reaction of the elements,[2] but it is more commonly prepared by carbothermal reduction of calcium phosphate:[3]

Ca3(PO4)2 + 8 C → Ca3P2 + 8 CO

The structure of the room temperature form of Ca3P2 has not been confirmed by X-ray crystallography. A high temperature phase has been characterized by Rietveld refinement]]. Ca2+ centers are octahedral.[2]

Uses

Metal phosphides are used as a rodenticide. A mixture of food and calcium phosphide is left where the rodents can eat it. The acid in the digestive system of the rodent reacts with the phosphide to generate the toxic gas phosphine. This method of vermin control has possible use in places where rodents immune to many of the common warfarin-type (anticoagulant) poisons have appeared. Other pesticides similar to calcium phosphide are zinc phosphide and aluminium phosphide.

Calcium phosphide is also used in fireworks, torpedoes, self-igniting naval pyrotechnic flares, and various water-activated ammunition. During the 1920s and 1930s, Charles Kingsford Smith used separate buoyant canisters of calcium carbide and calcium phosphide as naval flares lasting up to ten minutes. It is speculated that calcium phosphide—made by boiling bones in urine, within a closed vessel—was an ingredient of some ancient Greek fire formulas.[4]

Calcium phosphide is a common impurity in calcium carbide, which may cause the resulting phosphine-contaminated acetylene to ignite spontaneously.[5]

Safety considerations

On contact with acids or water, the material releases phosphine, which is toxic and is readily ignited.

See also

References

  1. ↑ Richard C. Ropp (31 December 2012). Encyclopedia of the Alkaline Earth Compounds. Newnes. pp. 231–. ISBN 978-0-444-59553-9.
  2. 1 2 Lilia S. Xie, Leslie M. Schoop, Elizabeth M. Seibel, Quinn D. Gibson, Weiwei Xie, Cava, Robert J. (2015). "A new form of Ca3P2 with a ring of Dirac nodes". APL Materials. 3: 083602. doi:10.1063/1.4926545.
  3. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
  4. ↑ Colin McEvedy (1992),The New Penguin Atlas of Medieval History, New York: Penguin.
  5. ↑ GOV, NOAA Office of Response and Restoration, US. "CALCIUM PHOSPHIDE | CAMEO Chemicals | NOAA". cameochemicals.noaa.gov. Retrieved 2016-08-26.
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