Understanding Xenon Difluoride

XeF₂, or Xenon Difluoride, is a potent chemical compound that was first discovered in 1962. It is known for its powerful fluoridating properties. In fact, XeF₂ was once considered a convenient replacement for elemental fluorine in addition reactions involving a double bond. The oxidation state of xenon in Xenon Difluoride is +2. Despite having a negligible vapour pressure at -78°, it rises to about 3 mm-Hg at room temperature. However, Xenon Difluoride is a hazardous chemical, reacting with water moisture to form hydrofluoric acid.

Also Known As – Difluoroxenon, Xenon fluoride

Synthesis of Xenon Difluoride – XeF₂

• • XeF₂ can be synthesized by heating a 2:1 mixture of xenon and fluorine at 400^oC in a sealed nickel vessel.

Xe + F₂ → XeF₂

• • Dioxygen difluoride can react with xenon at about 118^oC to yield XeF₂.

Xe + O₂F₂ → XeF₂ + O₂

Structure of Xenon Difluoride – XeF₂

Below is the structure of Xenon Difluoride.

Physical Properties of Xenon Difluoride – XeF₂

Applications of Xenon Difluoride – XeF₂

• It's used to fluorinate and oxidize the hetero element in an organometallic compound, without affecting the alkyl or aryl groups.
• It's used for the detection and determination of small quantities of iodine and iodide, as it oxidizes iodine to periodate.
• It's employed to kill bacteria, power lasers and tracers as an antiseptic. It's also preferred as fuel for ion engines in deep-space spacecraft.