Answer the question on basis of passage given below:
P block elements are placed in groups 13 to 18 of the periodic table. Their valence shell electronic configuration is \(ns^2\, \ np^{1-6}\). Group 16 of the p-block elements are known as the group of chalcogens having \(ns^2\, \ np^4\) as their general electronic configuration. They exhibit number of oxidation states but the stability of \(-2\) oxidation state decreases down the group. They are sometimes also known as group of chalcogens as the name is derived from the Greek word for brass and points to the association of sulphur and its congeners with copper. Their ionization enthalpy decreases down the group. Oxygen shows anomalous behaviour due to its small size and high electronegativity.
Which one is the correct electronic configuration of sulphur?
Answer & explanation
Correct answer: option 3
The correct answer is Option (3) → [Ne] 3s23p4
Sulphur has atomic number 16. Filling its 16 electrons in order of increasing energy:
\( \displaystyle \mathrm{1s^2\,2s^2\,2p^6\,3s^2\,3p^4} \)
The first ten electrons (1s2 2s2 2p6) are the neon core, so S = [Ne] 3s2 3p4, the group 16 pattern ns2np4 with n = 3. The other options have 14 electrons (silicon), 8 electrons (oxygen) and 18 electrons (argon).
Note: This question is from the pre-rationalised NCERT book (2022-23). The topic is not there in the latest NCERT book (2026-27), and it is also out of the CUET 2026 syllabus.