Sulphur (S) is a non-metallic element with Atomic Number 16. It belongs to Group 16 (Chalcogens) and Period 3 of the Periodic Table. Knowing its electronic configuration explains its chemical behaviour, valency, and bonding properties.
Sulphur's most common allotrope is Rhombic Sulphur (S₈), which consists of rings of 8 sulphur atoms. This is why its chemical formula is often written as S₈.
Sulphur has 16 electrons distributed across 3 shells:
| Shell | Name | Electrons |
|---|---|---|
| 1st | K | 2 |
| 2nd | L | 8 |
| 3rd | M | 6 |
Representation: S: 2, 8, 6
This is the simplest way to remember sulphur's electronic arrangement.
In the orbital notation, the 16 electrons of sulphur are distributed as:
1s² 2s² 2p⁶ 3s² 3p⁴
This means:
Valency: Sulphur has 6 electrons in its outermost shell (valence electrons). It needs 2 more electrons to complete the octet, giving it a valency of 2 (as in H₂S). It can also show valencies of 4 and 6 due to its expandable d-orbitals.
In its ground state, sulphur has 2 unpaired electrons giving a valency of 2 (e.g., H₂S). However, sulphur can promote electrons to empty 3d orbitals, creating 4 or 6 unpaired electrons, explaining its variable valency of 4 (e.g., SO₂) and 6 (e.g., SO₃, H₂SO₄).
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