All of the noble gases have filled s- and p-orbitals, giving them 8 outer shell electrons.
The outer shell of electrons in noble gases is full.
Noble gases do not like giving up electrons. There are 2 electrons in the outer shell of helium and 8 electrons in the outer shell of the other noble gases (group 18 of the periodic table), representing filled shells.
Each noble gas has an 'octet' of electrons, meaning a full outer shell of 8 electrons, except for Helium which only needs 2 electrons to fill the outer shell.
Noble gases have a full outer shell, meaning that they have no valence electrons and have 8 electrons in their outer shell. If the outer shell is full they do not need electrons, so they would not want to bond with another element to form a compound.
Yes they do, because, for example, neon has 2 electrons in its inner shell and 8 on its outer shell; these shells are both full. Helium, the lightest of the noble gases, has only 2 electrons, but that completes it only shell. All the other noble gases have 8 electrons in their outer shell, which is a stable arrangement.
All noble gases have completely filled outer shell with 8 electrons (only helium has 2 valence electrons)
8 electrons (except for helium which has 2)
Having the outer shell of electrons filled noble gases are very stable.
The innermost shell contains a maximum of 2 electrons, therefore like the other noble gases, it has a full outer shell. The other noble gases all have eight in their outer shells.