Lithium phosphide

Today, we want to talk about Lithium phosphide and how it has impacted society in recent years. Lithium phosphide has become a topic of interest for many people, as its influence has spread to different areas, from technology to fashion. In this article, we will explore some key aspects related to Lithium phosphide, including its history, its evolution over time, and its relevance today. In addition, we will analyze how Lithium phosphide has affected different sectors and has generated discussions around its importance in modern society. Join us on this journey to discover more about Lithium phosphide and its impact on the world today!

Lithium phosphide
Names
Other names
Trilithium phosphide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.031.824 Edit this at Wikidata
EC Number
  • 235-020-0
  • InChI=1S/3Li.H2P/h;;;1H2/q3*+1;-1
    Key: IEAMEDSGNMSUND-UHFFFAOYSA-N
  • ...
Properties
Li3P
Molar mass 51.79 g·mol−1
Appearance Red-brown crystals
Density 1.43 g/cm3
Reacts
Structure
cubic
Related compounds
Other anions
Other cations
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).

Lithium phosphide is an inorganic compound of lithium and phosphorus with the chemical formula Li3P. This dark colored compound is formally the lithium salt of phosphine, consisting of lithium cations Li+ and phosphide anions P3−. It is hazardous to handle because of its high reactivity toward air.[1]

Synthesis

Heating red phosphorus and lithium in an argon atmosphere:[1]

12 Li + P4 → 4 Li3P

Reaction of monolithium phosphide and lithium:

LiP + 2 Li → Li3P

Physical and chemical properties

Lithium phosphide forms red-brown crystals of hexagonal systems, space group P63/mmc,[2] cell parameters a = 0.4264 nm, c = 0.7579 nm, Z = 2.[3][4]

The compound is a very strong base, and reacts with water to release phosphine:[5]

Li3P + 3 H2O → 3 LiOH + PH3

Uses

The compound is proposed to be used as a potential electrolyte for solid-state devices.[6]

Reaction of lithium with red phosphorus at 870 °C gives Li3P7.[7]

Further reading

  • Nazri, Gholamabbas (1 April 1989). "Preparation, structure and ionic conductivity of lithium phosphide". Solid State Ionics. 34 (1–2): 97–102. doi:10.1016/0167-2738(89)90438-4.

Safety

Alkali metal phosphides are dangerous compounds when exposed to oxygen or moisture.[8]

References

  1. ^ a b E. Donges (1963). "Phosphides, Arsenides, Antimonides and Bismuthides of Alkali Metals from the Elements". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 985.
  2. ^ "mp-736: Li3P (hexagonal, P6_3/mmc, 194)". materialsproject.org. Retrieved 10 December 2021.
  3. ^ Seel, Max; Pandey, Ravi (1990). "Band Structure and Electronic Properties of Lithium Phosphide Li3P". MRS Proceedings. 210. doi:10.1557/PROC-210-155. Retrieved 10 December 2021.
  4. ^ Donnay, Joseph Désiré Hubert (1963). Crystal Data; Determinative Tables. American Crystallographic Association. p. 765. Retrieved 10 December 2021.
  5. ^ Dong, Yongkwan; DiSalvo, Francis J. (15 April 2007). "Reinvestigation of trilithium phosphide, Li 3 P". Acta Crystallographica Section E. 63 (4): i97 – i98. doi:10.1107/S1600536807008422.
  6. ^ Wan, Chaoying; Huang, Xingyi; Bowen, Chris (23 June 2021). Two-dimensional Inorganic Nanomaterials for Conductive Polymer Nanocomposites. Royal Society of Chemistry. ISBN 978-1-83916-260-2. Retrieved 10 December 2021.
  7. ^ Manriquez, V.; Hönle, W.; von Schnering, H. G. (1986). "Zur Chemie und Strukturchemie von Phosphiden und Polyphosphiden. 42. Trilithiumheptaphosphid Li3P7: Darstellung, Struktur und Eigenschaften". Zeitschrift für Anorganische und Allgemeine Chemie. 539 (8): 95–109. doi:10.1002/zaac.19865390810.
  8. ^ Toxic Substances Control Act (TSCA) Chemical Substance Inventory. U.S. Government Printing Office. 1979. p. 9. Retrieved 10 December 2021.