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It was mentioned in section today that Xenon is the only noble gas that can form covalent bonds. Why is this so? Why are other noble gases with d and f orbitals unable to do this?
I could be wrong, but from my understanding, Xe has a larger atomic radius compared to the other noble gases above the element. I wondered why Radon couldn't form bonds despite the large radius like Xenon, but because Radon is radioactive, that would mean that the element is unstable and would be unlikely to form bonds.
I think it's because the large radius of the atom negates part of the hold that the nucleus has on the valence electrons. When combined with a very electronegative atom, it can form bonds.
Xe can form bonds because it has a very large atomic radius compared to other noble gases meaning that the ionization energy of the atom for the outermost electrons is relatively minimal, minimal enough to allow it to create bonds with atoms that have relatively high electronegativity.
With the other noble gasses, the valence shell is full and close to the nucleus so it is very difficult to remove an electron but as others mentioned having the valence electrons farther from the nucleus means it is easier for them to get pulled away.
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