Question

Complete hydrolysis of $Xe{F}_4$ and $Xe{F}_6$ results in the formation of $Xe{O}_3$ . Explain.

Answer 1

Hint: A chemical reaction in which a molecule of water is added to a substance is known as hydrolysis. When this happens, both the material and the water molecule will break into two. One fragment of the target molecule (or parent molecule) gains a hydrogen ion in certain reactions.

Complete answer:
At 298K, $Xe{F}_4$, and $Xe{F}_6$ are colourless crystalline solids that are easily sublime. They're fluorinating agents with a lot of energy. Also traces of water are enough to hydrolyse them.
Hydrolysis of $Xe{F}_6$:
One of the three binary fluorides generated by xenon is $Xe{F}_6$. When $Xe{F}_6$ is completely hydrolysed, $Xe{O}_3$ (xenon trioxide) is generated. In solution, xenon trioxide is highly volatile and serves as a potent oxidizer.
$Xe{F}_6+3H_{2}O\to Xe{O}_3+6HF$
Hydrolysis of $Xe{F}_4$:
As xenon tetrafluoride combines with water, it produces xenon, oxygen, hydrofluoric acid, and a highly soluble xenon species. When the solution is evaporated, a white, crystal-line material known as xenon $(VI)$ oxide, XeO$(III)$, is formed . When it comes into contact with organic products, it becomes dangerously explosive.
$6Xe{F}_4+12H_{2}O\to 4Xe+2Xe{O}_3+24HF+3O_2$
As $Xe{F}_4$ is partially hydrolyzed, it releases xenon oxydifluoride ($XeO{F}_2$).
$Xe{F}_4+H_{2}O\to XeO{F}_2+2HF$

Note:
Xenon can be split into three fluorides: $Xe{F}_2$, $Xe{F}_4$, and $Xe{F}_6$. In the right laboratory conditions, this can be achieved by a direct reaction of xenon and fluorine. In its +6 oxidation state, xenon trioxide is an acidic xenon compound. It's a powerful oxidizer that steadily releases oxygen from water, which is accelerated by exposure to sunlight.