The correct answer is option 2. \(NeF_2\).
Noble gases, which include helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn), are generally known for their inert behavior. Inert gases typically do not readily form compounds under normal conditions because they have a full complement of electrons in their outer electron shells, making them stable.
Let us analyze each compound:
1. \(XeOF_4\) (Xenon oxytetrafluoride): This compound exists and has been synthesized. Xenon can expand its valence shell due to its large atomic size, and under certain conditions, it can form compounds.
2. \(NeF_2\) (Neon difluoride): Neon is a noble gas with a completely filled outer electron shell, and it is generally unreactive under normal conditions. The synthesis of neon compounds, especially difluorides, is highly unlikely.
3. \(XeF_2\) (Xenon difluoride): This compound exists and is well known. Xenon can undergo hybridization to accommodate additional electron pairs and form compounds with fluorine.
4. \(XeF_6\) (Xenon hexafluoride): This compound also exists and has been synthesized. Xenon hexafluoride is an example of a noble gas compound where xenon exhibits an expanded valence shell.
In summary, while \(XeOF_4\), \(XeF_2\), and \(XeF_6\) are known compounds involving xenon, \(NeF_2\) is not a likely compound due to neon's inert nature. Neon typically does not form stable compounds under normal conditions.
Therefore, the compound that is least likely to exist is:(2) \(NeF_2\) |
