Phosphinate

Today we are going to talk about Phosphinate, a topic that has generated interest and debate in contemporary society. Phosphinate is a topic that has been the subject of study and analysis in different fields, from psychology to politics, including popular culture and technology. This article seeks to offer a comprehensive and updated vision of Phosphinate, addressing its different facets and its impact on daily life. Along these lines we will explore the most relevant aspects of Phosphinate, examining its repercussions and possible solutions. Without a doubt, Phosphinate is a topic that does not leave anyone indifferent, and it is crucial to understand it in depth to better understand the world in which we live.

Phosphinate
Sodium hypophosphite
Identifiers
3D model (JSmol)
ChemSpider
UNII
  • InChI=1S/H3O2P/c1-3-2/h3H2,(H,1,2)/p-1
    Key: ACVYVLVWPXVTIT-UHFFFAOYSA-M
  • =O
Properties
H2O2P−
Molar mass 64.988 g·mol−1
Related compounds
Related compounds
 phosphite; phosphine oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).

Phosphinates or hypophosphites are a class of phosphorus compounds conceptually based on the structure of hypophosphorous acid. IUPAC prefers the term phosphinate in all cases, however in practice hypophosphite is usually used to describe inorganic species (e.g. sodium hypophosphite), while phosphinate typically refers to organophosphorus species.

Hypophosphites

The hypophosphite ion is (H
2PO
2)−
. The salts are prepared by heating white phosphorus in warm aqueous alkali e.g. Ca(OH)2:[1]

P4 + 2 Ca(OH)2 + 4 H2O → 2 Ca(H2PO2)2 + 2 H2

Hypophosphites are reducing agents:[1]

(H
2PO
2)−
 + 3 OH− → (HPO
3)2−
 + 2 H2O + 2 e−

Hypophosphites are used in electroless nickel plating as the reducing agent to deposit for example Ni metal from Ni salts.[1] The hypophosphite ion is thermodynamically unstable, and disproportionates on heating to phosphine and phosphate salts:

2 H
2PO
2−
 → PH3 + HPO
42−

See also

References

  1. ^ a b c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 512. ISBN 978-0-08-037941-8.