Argon fluorohydride

Today, Argon fluorohydride is a topic that has acquired great relevance in different areas. Both in personal life and in the work environment, Argon fluorohydride has generated a significant impact on the way people interact and function in their daily lives. Since its emergence, Argon fluorohydride has been the subject of study, debate and analysis, which has given rise to a multiplicity of perspectives and approaches on its importance and repercussions. In this article, we will explore various facets of Argon fluorohydride, from its origin to its evolution today, in order to better understand its influence on our society.

Argon fluorohydride
Argon fluorohydride
Argon fluorohydride
Names
Other names
Argon hydrofluoride
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/ArFH/c1-2/h1H checkY
    Key: HEPJAPHKUAGBIG-UHFFFAOYSA-N checkY
  • InChI=1/ArFH/c1-2/h1H
    Key: HEPJAPHKUAGBIG-UHFFFAOYAL
  • F
Properties
HArF
Molar mass 59.954 g/mol
Appearance Unknown
Density Unknown
Melting point −256 °C (−428.8 °F; 17.1 K) (decomposes)
Unknown
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa).
checkY verify (what is checkY☒N ?)

Argon fluorohydride (systematically named fluoridohydridoargon) or argon hydrofluoride is an inorganic compound with the chemical formula HArF (also written ArHF). It is a compound of the chemical element argon.

Discovery

The discovery of this argon compound is credited to a group of Finnish scientists, led by Markku Räsänen.[1] On 24 August 2000, in the journal Nature, they announced their discovery of argon fluorohydride.[2] This discovery caused the recognition that argon could form weakly bound compounds, even though it was not the first compound made with noble gases.[3]

Synthesis

This chemical was synthesized by mixing argon and hydrogen fluoride on a caesium iodide surface at 8 K (−265 °C), and exposing the mixture to ultraviolet radiation. This caused the gases to combine.

The infrared spectrum of the resulting gas mixture shows that it definitely contains chemical bonds, albeit very weak ones; thus, it is argon fluorohydride, and not a supermolecule or a mixture of argon and hydrogen fluoride. Its chemical bonds are stable only if the substance is kept at temperatures below 27 K (−246 °C); upon warming, it decomposes into argon and hydrogen fluoride.[2]

References

  1. ^ Räsänen, Markku (17 December 2013). "Argon out of thin air". Nature Chemistry. 6 (1): 82. doi:10.1038/nchem.1825. PMID 24345939.
  2. ^ a b Khriachtchev, Leonid; Mika Pettersson; Nino Runeberg; Jan Lundell; Markku Räsänen (24 August 2000). "A stable argon compound". Nature. 406 (6798): 874–876. Bibcode:2000Natur.406..874K. doi:10.1038/35022551. PMID 10972285. S2CID 4382128.
  3. ^ Perkins, Sid (29 April 2003). ""HArF! Argon's not so noble after all – researchers make argon fluorohydride"". Science News. Retrieved 24 April 2024.

Further reading

  • Emsley, John (2001). Nature's Building Blocks: An A–Z Guide to the Elements. Oxford: Oxford University Press. ISBN 0-19-850341-5.