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 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?

\([Ne] 3s^23p^4\)

The correct answer is option 3. \([Ne] 3s^23p^4\).

To explain the electronic configuration of sulfur, let us break down the process of how electrons are distributed in its atomic orbitals:

Sulfur (S) has an atomic number of 16. This means sulfur has 16 electrons in its neutral state. The electron configuration describes how these electrons are distributed across various atomic orbitals, following the principles of quantum mechanics. The order in which electrons fill orbitals is determined by the Aufbau principle, Hund's rule, and the Pauli exclusion principle.

Filling the Orbitals

First Shell (K shell, \(n=1\)):

1s Orbital: This shell can hold a maximum of 2 electrons.

Configuration: \(1s^2\)

Second Shell (L shell, \(n=2\)):

2s Orbital: Can hold up to 2 electrons.

2p Orbitals: Can hold up to 6 electrons.

Configuration: \(2s^2 2p^6\)

Third Shell (M shell, \(n=3\)):

3s Orbital: Can hold up to 2 electrons.

3p Orbitals: Can hold up to 6 electrons.

Since sulfur has only 16 electrons in total, the remaining 6 electrons will go into the 3p orbitals.

Configuration: \(3s^2 3p^4\)

To simplify the configuration, we use the nearest noble gas core as a reference. For sulfur, the nearest noble gas preceding it in the periodic table is Neon (Ne), which has an atomic number of 10 and an electronic configuration of \(1s^2 2s^2 2p^6\). Thus, the configuration for sulfur can be written as:

[Ne]*for the core electrons (representing the configuration up to 2s² 2p⁶)

Followed by the configuration of the remaining electrons in the third shell: 3s² 3p⁴

Thus, the complete electronic configuration of sulfur is:

\(1s^2 2s^2 2p^6 3s^2 3p^4\)

In condensed notation, this is: [Ne] 3s² 3p⁴

Thus, the correct choice for sulfur’s electronic configuration is indeed: 3. [Ne] 3s² 3p⁴