Noble gases have very low boiling points. Why?

How are xenon fluorides $XeF_2$,$XeF_4$ and $XeF_6$ obtained?

The density of nitrogen obtained by the liquefaction of air is higher than that of nitrogen obtained by chemical reactions from nitrogenous compounds. This is due to the presence of which gas in the atmospheric nitrogen?

Which of the following statements is $NOT$ true for noble gases?

$Xe_{(g)} + 3F_{2(g)} \xrightarrow{573 \ K, 60-70 \ bar} XeF_{6(s)}$ ($1:20$ molar ratio).
$XeF_6 + H_2O \rightarrow XeOF_4 + 2HF$ $(Y)$
$XeF_6 + 3H_2O \rightarrow XeO_3 + 6HF$ $(Z)$
The correct statements regarding $Y$ and $Z$ are:
$I$. $Y$ has square pyramidal geometry
$II$. $Y$ has linear geometry
$III$. $Z$ has $3 \sigma, 3 \pi$ bonds and $1$ lone pair of electrons on the central atom
$IV$. $Z$ has tetrahedral geometry

Which of the following fluorides of xenon is impossible?