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, $XeF_4$, and $XeF_6$ 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.
$Xe{F_6} + 3{H_2}O \to Xe{O_3} + 6HF$
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.
$6Xe{F_4} + 12{H_2}O \to 4Xe + 2Xe{O_3} + 24HF + 3{O_2}$
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: $XeF_2$, $XeF_4$, and $XeF_6$. 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.