* Electronic Configuration: Sulfur has 6 valence electrons (electrons in its outermost shell).
* Octet Rule: Sulfur tends to gain or share electrons to achieve a stable octet (8 electrons) in its outer shell.
Common Valencies of Sulfur:
* +2: Sulfur can lose 2 electrons, forming cations like S²⁺ (found in some sulfides).
* +4: Sulfur can lose 4 electrons, forming cations like S⁴⁺ (found in some sulfur oxides).
* +6: Sulfur can lose 6 electrons, forming cations like S⁶⁺ (found in some sulfur compounds like sulfuric acid).
* -2: Sulfur can gain 2 electrons, forming anions like S²⁻ (found in sulfides like sodium sulfide).
Examples:
* Sulfides: In compounds like H₂S (hydrogen sulfide), sulfur has a valency of -2.
* Sulfur dioxide (SO₂): Sulfur has a valency of +4.
* Sulfur trioxide (SO₃): Sulfur has a valency of +6.
* Sulfuric acid (H₂SO₄): Sulfur has a valency of +6.
Important Note: The valency of sulfur is influenced by the electronegativity of the other elements it bonds with.
