Why wont hydrogen bond with other noble gases?

Answer 1

First - Hydrogen isn't a noble gas.

Actually, no elements will bond with noble gases except under extreme conditions. Chemicals bond by either sharing or trading electrons. Noble gases have all of the electrons they need, and hydrogen atoms have one extra electron, thus noble gases don't want to bond.

In 1933 Linus Pauling predicted that the heavier noble gases would be able to form compounds with fluorine and oxygen. Specifically, he predicted the existence of krypton hexafluoride (KrF6) and xenon hexafluoride (XeF6), speculated that XeF8 might exist as an unstable compound, and suggested that xenic acid would form perxenate salts. These predictions proved quite accurate, although subsequent predictions for XeF8 indicated that it would be not only thermodynamically unstable, but kinematically unstable. As an example of the extreme conditions usually required to make such molecules, Xenon hexafluoride can be prepared by long-term heating of XeF2 at about 300°C and pressure 6 MPa (60 atmospheres).

Answer 2

Hydrogen does not typically form stable hydrogen bonds with noble gases because noble gases have complete electron shells and are already stable. Hydrogen bonds usually occur between hydrogen and more electronegative atoms like oxygen, nitrogen, or fluorine.