Question

ground state electronic configuration of sulphide ion ?why​

Answer 1

Explanation:

A good starting point when looking for the electron configuration of an ion is the electron configuration of the neutral atom.
In your case, the neutral atom is sulfur, S, which is located in period 3, group 16 of the periodic table. Sulfur's has an atomic number equal to 16, which means that a neutral sulfur atom has a total of 16electrons surrounding its nucleus.
The electron configuration of a neutral sulfur atom will thus be

S: 1s22s22p63s23p4

Now, the sulfide anion, S2−, is formed when two electrons are added to a neutral sulfur atom.
As you can see in the configuration of the neutral atom, these two electrons will be added to the 3p-orbitals, which can hold a maximum of six electrons between them.
The electron configuration of the sulfide anion will thus be

S2−:a1s22s22p63s23p6

The noble gas shorthand notation for the sulfide anion will use the electron configuration of neon, the noble gas that comes immediately before sulfur in the periodic table.

✅

Answer 2

Explanation:

Therefore the sulfur electron configuration will be 1s22s22p63s23p4. The configuration notation provides an easy way for scientists to write and communicate how electrons are arranged around the nucleus of an atom.

Mark as Brainlist