Which of the following represents the correct pair of the molecular formula of a xenon compound and the hybridization of xenon?

Xenon hexafluoride on partial hydrolysis produces compounds $X$ and $Y$. Compounds $X$ and $Y$ and the oxidation state of $Xe$ are respectively

Ionisation potential values of noble gases decrease down the group with increase in atomic size. Xenon forms binary fluorides by the direct reaction of elements. Identify the correct statement$(s)$ from below.

$Xe_{(g)} + 2 F_{2(g)} \xrightarrow[7 \text{ bar }]{873 \text{ K}} XeF_{4(s)}$
The ratio of $Xe : F_2$ required in the above reaction is

The type of hybridisation and number of lone pair$(s)$ of electrons of $Xe$ in $XeOF_4$ respectively are

Balance the following equation: $XeF_{6} + H_{2}O \rightarrow XeO_{2}F_{2} + HF$