[Ne]3s23p4
[noble gas]ns2 np6
By acquiring noble gas configuration elements become stable .
Sulfur atoms will gain two electrons in order to achieve a noble gas electron configuration. A sulfide ion has the formula S2-.
Aluminum is [Ne]3s23p1 Sulfur is [Ne]3s23p4
it only fills the S sublevel
Noble gases have a stable electron configuration. So they are less reactive.
All of the noble gasses have full outer electron shells - rendering them extremely nonreactive. Their electron configuration is what places them in the group on the periodic table that we have designated "noble gases".
The group of elements that have a stable electron configuration are the noble gases.
Sulfide, S2-
nitrogen will get noble gas configuration by adding three more electrons.
Helium's electron configuration is 1s2. Neon's electron configuration is 1s22s22p6. All of the rest of the noble gases, like neon, have the maximum number of electrons in their outermost s and p orbitals (valence shells), which is eight.
K+And the K ion configuration is 1s2 2s2 2p6 3s2 3p6Noble gases have the configuration up to 3p6Pseudo noble gases have it up to 3d10