Yes. S2- has the electronic configuration of argon
Sulfide, S2-
Krypton (Kr) has the same electron configuration as S2, which is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6.
The noble gas that is isoelectronic with S2- is Argon. Both S2- and Argon have 18 electrons.
1s22s22p6
The stable ions of all the elements except the Transition metals, Actinide, and Lanthanide series (that is the d and f block elements) form stable ions that are isoelectronic to a nobel gas by gaining or losing electrons in order to achieve an s2 p6 stable octet. For example, sodium will lose one electron to have the same electron configuration as neon, while nitrogen will gain three electrons to become isoelectronic to neon.
Na, Rb, Al3+, and S2- do not have a noble gas configuration as they do not have the complete outer shell of electrons like a noble gas. O2, Br, Ca, and O2- have noble gas configurations as they either have a complete outer shell of electrons or have gained/lost electrons to achieve a stable noble gas configuration.
Sulfide, S2-
Krypton (Kr) has the same electron configuration as S2, which is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6.
The noble gas that is isoelectronic with S2- is Argon. Both S2- and Argon have 18 electrons.
Sulfur atoms will gain two electrons in order to achieve a noble gas electron configuration. A sulfide ion has the formula S2-.
1s22s22p6
S2- ion: [Ne]3s23p6
A sulfide ion (S2-) must gain two electrons to achieve a noble gas electron configuration, similar to that of a stable, inert gas such as argon. This transfer allows the sulfide ion to fill its valence shell with eight electrons, satisfying the octet rule.
The stable ions of all the elements except the Transition metals, Actinide, and Lanthanide series (that is the d and f block elements) form stable ions that are isoelectronic to a nobel gas by gaining or losing electrons in order to achieve an s2 p6 stable octet. For example, sodium will lose one electron to have the same electron configuration as neon, while nitrogen will gain three electrons to become isoelectronic to neon.
When sulfur gains electrons, it forms the sulfide ion with a 2- charge, represented as S2-. When sulfur loses electrons, it forms the sulfide ion with a 2+ charge, represented as S2+.
A sulfide ion will have a charge of -2. This is because sulfur is in Group 6 of the periodic table and typically forms ions by gaining two electrons to achieve a stable, noble gas electron configuration.
Sulfur gains two electrons to attain a noble gas configuration, which is the electron configuration of argon. This allows sulfur to have a stable octet of electrons in its outer shell and achieve a more stable electron configuration.