What accounts for the stability of the noble gas electron configuration?

Answer 1

The outer, or valence, shells of the noble gases are completely filled, so that they neither donate to nor accept electrons from other atoms. As a result, noble gas atoms cannot form chemical bonds, so they remain pure. Most elements do not have filled outer shells. Atoms that have nearly full outer shells readily accept electrons, and those with nearly empty outer shells readily donate electrons. "Donated" electrons and "accepted" electrons are simply electrons that are attracted to the nuclei of two atoms. That shared attraction holds the two atoms together. Thus most elements can form chemical bonds.

Answer 2

On the contrary, noble gases are not likley to form bonds.

Noble gases have an octet of electrons in their outer shell.

Some compounds of Ar, Kr, Xe and Rn are known but these are very reactive and in some cases very unstable.

Answer 3

The stability of noble gas electron configurations is due to their full outer electron shells, which result in low reactivity and a lack of tendency to gain or lose electrons. This full outer shell configuration gives them a high level of stability and makes them chemically inert.

Answer 4

the tendency toward a complete octet of electrons in a bonded atom reflects the natural tendency for a system to move to the lowest energy state possible.

Answer 5

Because of their electronic structure that makes them unreactive

Answer 6

none