Zinc phosphide

Zinc phosphide[1]
Names
Other names
trizinc diphosphide
Identifiers
1314-84-7 (Zn
2P
3)
 
12037-79-5 (ZnP
2)
 
51810-70-9 (Zn
xP
x) 
ChemSpider 11344765 Yes
Jmol-3D images Image
UNII 813396S1PC Yes
Properties
Zn3P2
Molar mass 258.12 g/mol
Appearance gray tetragonal crystals
Density 4.55 g/cm3
Melting point 1,160 °C (2,120 °F; 1,430 K)
insoluble
Solubility insoluble in ethanol, soluble in benzene, reacts with acids
Structure
Crystal structure Tetragonal, tP40
Space group P42/nmc, No. 137
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
  verify (what is: Yes/?)
Infobox references

Zinc phosphide (Zn3P2) is the inorganic chemical compound. It is a grey solid, although commercial samples are often dark or even black. It is used as a rodenticide.[2] Zn3P2 is a semiconductor with a direct band gap of 1.5 eV.[3] and may have applications in photovoltaic cells.[4] A second zinc phosphide is known, with the stoichiometry ZnP2.

Synthesis and reactions

Zinc phosphide can be prepared by the reaction of zinc with phosphorus; however, for critical applications, additional processing to remove arsenic compounds may be needed.[5]

3 Zn + 2 P → Zn3P2

Another method of preparation include reacting tri-n-octylphosphine with dimethylzinc.[6]


Zinc phosphide reacts with water to produce phosphine (PH3) and zinc hydroxide (Zn(OH)2):

Zn3P2 + 6 H2O → 2 PH3 + 3 Zn(OH)2

Structure

Zn3P2 has two forms, a room temperature tetragonal form which converts to a cubic form at around 845 °C. [7] In the room temperature form there are discrete P atoms, zinc atoms are tetrahedrally coordinated and phosphorus six coordinate, with zinc atoms at 6 of the vertices of a distorted cube.[8] ZnP2 has two forms a lower temperature red tetragonal form and a black monoclinic form.[7] In both of these there are chains of P atoms, helical in the tetragonal, semi-spiral in the monoclinic.[9]

Rodenticide

Metal phosphides have been used as rodenticides. A mixture of food and zinc 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 phosphine gas. This method of vermin control has possible use in places where rodents immune to other common poisons. Other pesticides similar to zinc phosphide are aluminium phosphide and calcium phosphide.

Zinc phosphide is typically added to rodent baits in amount of around 0.75-2%. Such baits have strong, pungent garlic-like odor characteristic for phosphine liberated by hydrolysis. The odor attracts rodents, but has a repulsive effect on other animals; birds, notably wild turkeys, are not sensitive to the smell. The baits have to contain sufficient amount of zinc phosphide in sufficiently attractive food in order to kill rodents in a single serving; a sublethal dose may cause aversion towards zinc-phosphide baits encountered by surviving rodents in the future.

Rodenticide-grade zinc phosphide usually comes as a black powder containing 75% of zinc phosphide and 25% of antimony potassium tartrate, an emetic to cause vomiting if the material is accidentally ingested by humans or domestic animals. However, it is still effective against rats, mice, guinea pigs and rabbits, none of which have a vomiting reflex.[10]

Zinc phosphide use in New Zealand

The New Zealand Environmental Protection Authority has approved the import and manufacture of Microencapsulated Zinc Phosphide (MZP Paste) for the ground control of possums. The application was made by Pest Tech Limited, with support from Connovation Ltd, Lincoln University and the Animal Health Board. It will be used as an additional vertebrate poison in certain situations. Unlike 1080 poison, it cannot be used for aerial application.[11]

Safety

Zinc phosphide is highly toxic.

References

  1. ↑ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, FL: CRC Press. pp. 4–100. ISBN 0-8493-0594-2.
  2. ↑ Bettermann, G.; Krause, W.; Riess, G.; Hofmann, T. (2002). "Phosphorus Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_527.
  3. ↑ Kimball, Gregory M.; Müller, Astrid M.; Lewis, Nathan S.; Atwater, Harry A. (2009). "Photoluminescence-based measurements of the energy gap and diffusion length of Zn[sub 3]P[sub 2]". Applied Physics Letters 95 (11): 112103. doi:10.1063/1.3225151. ISSN 0003-6951.
  4. ↑ Specialist Periodical Reports, Photochemistry, 1981, Royal Society of Chemistry, ISBN 9780851860954
  5. ↑ F. Wagenknecht and R. Juza "Zinc Phosphides" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1080-1.
  6. ↑ Luber, Erik J.; Mobarok, Md Hosnay; Buriak, Jillian M. (2013). "Solution-Processed Zinc Phosphide (α-Zn3P2) Colloidal Semiconducting Nanocrystals for Thin Film Photovoltaic Applications". ACS Nano 7 (9): 8136–8146. doi:10.1021/nn4034234. ISSN 1936-0851.
  7. ↑ 7.0 7.1 Evgeniĭ I︠U︡rʹevich Tonkov, 1992, High Pressure Phase Transformations: A Handbook, Vol 2, Gordon and Breach Science Publishers , ISBN 9782881247590
  8. ↑ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
  9. ↑ Hans Georg von Schnering and Wolfgang Hönle, 1994, Phosphides: Solid State Chemistry, Encyclopedia of Inorganic chemistry, Ed. R Bruce King, John Wiley and Sons, ISBN 0-471-93620-0
  10. ↑ "Why rats can't vomit". Ratbehavior.org. Retrieved 2013-08-17.
  11. ↑ Environment Risk Management Authority New Zealand. "Zinc phosphide pest poison approved with controls". Retrieved 2011-08-14.

External links