# Question #b2eb0

Noble gas configuration refers to the state of having eight electrons in the valence shell of the electron configuration (${s}^{2} {p}^{6}$).
Non-metals typically are missing electrons in the p orbitals. Fluorine for example has an electron configuration of $1 {s}^{2} 2 {s}^{2} 2 {p}^{5}$. Fluorine is missing one electron in the 2p orbital. Fluorine will readily accept an electron in order to fill the 2p orbital and fill the valence shell. In doing this the fluorine atom becomes a -1 anion (${F}^{- 1}$.
And the new electron configuration becomes $1 {s}^{2} 2 {s}^{2} 2 {p}^{5}$, the same as the noble gas neon.
Sulfur has an electron configuration of $1 {s}^{2} 2 {s}^{2} 2 {p}^{6} 3 {s}^{2} 3 {p}^{4}$.
Sulfur will readily add two electrons to fill the valence shell (3s and 3p). This will make sulfur an ${S}^{- 2}$ anion with an electron configuration of $1 {s}^{2} 2 {s}^{2} 2 {p}^{6} 3 {s}^{2} 3 {p}^{6}$, the same as the noble gas argon.