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Noble gases or inert gases have electron configurations that are very stable.

Helium 1s2

Neon [He] 2s2 2p6

Argon [Ne] 3s2 3p6

Krypton [Ar] 3d10 4s2 4p6

Xenon [Kr] 5s2 4d10 5p6

Radon [Xe] 4f14 5d10 6s2 6p6

Helium has a full energy shell, as does neon. The rest have partially filled outer shells but with the s2p6 configuration seen in neon (the "octet")

What this tells you is that He, Ne should be really stable but that the others may be persuaded form compounds, if you tried hard enough. Compounds of xenon were the first to be made in the 1960s, the xenon fluorides. Compounds for Krypton are known and very recently some really unstable compounds of Argon.

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Q: Why do the atoms of a noble gas not combine to form molecules?
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