Why dont noble gases bond with other elements?

Answer 1

Noble gases have stable octets, meaning they have 8 electrons on their outest shell, which is the max electrons the shell can hold. Since noble gases' outer shells are full, they cannot share or gain electrons from other atoms therefore they do not bond.

Answer 2

Looking at the Periodic Table we can tell many things, one of the most important is the number of valence electrons available for bonding. The number of valence electrons available for bonding in the noble gases are 8, which happens to also be the maximum number of electrons available for bonding. As such, they do not naturally form any compounds because they have a full octet (8 electrons).

Answer 3

The compounds forming ability of any element depends upon its electronic configuration.

Those elements which have incomplete octet (or rather incompletely filled outermost shell) will form compounds in order to complete it, as this configuration offers maximum stability.

But noble gases already have completed octet.

Note that from 1960 up today more than hundred compounds of noble gases were prepared.

Answer 4

Because they already have a stable electronic configuration with 8 electrons in their outermost orbit.

Answer 5

atoms with eight valence electrons are stable. such atoms are unlikely to transfer electrons with other atoms.

Answer 6

Noble gases have full valence electron shells, making them extremely stable and unreactive. Due to this stability, they do not readily form chemical bonds with other elements.