Statement - I : Xenon fluorides are well known and stable but the corresponding chlorides have not been reported.
Statement - II : Xe-F bond is more strong than Xe-Cl bond and F₂ molecule has low bond dissociation energy than that of Cl₂ molecule.

Statement I is partially true because some xenon chlorides have been reported, although they are generally less stable than the corresponding xenon fluorides. The most well-known xenon chloride is XeCl₂, which is a pale-yellow solid at room temperature and is somewhat unstable. Other xenon chlorides, such as XeCl₄ and XeCl₆, have also been reported, but they are even less stable than XeCl₂.

Statement II is true because the Xe-F bond is stronger than the Xe-Cl bond. This is because fluorine is more electronegative than chlorine, which means it attracts electrons more strongly and forms a stronger bond with xenon. Additionally, the F₂ molecule has a lower bond dissociation energy than the Cl₂ molecule, which means that it takes less energy to break the F-F bond than the Cl-Cl bond. This also contributes to the greater strength of the Xe-F bond compared to the Xe-Cl bond.