* Electron Configuration: Sulfur has 6 valence electrons (electrons in its outermost shell). To become stable, it needs 8 valence electrons (like the noble gas Argon).
* Octet Rule: The octet rule states that atoms tend to gain, lose, or share electrons to achieve a full outer shell of 8 electrons.
* Electronegativity: Sulfur is more electronegative than many metals. This means it has a stronger attraction for electrons.
* Ionic Bond Formation: When sulfur encounters a metal (like sodium, Na), which has a lower electronegativity and only 1 valence electron, sulfur "steals" that electron. This leaves sulfur with 7 electrons in its outer shell, and the metal (like sodium) becomes positively charged.
The result is that sulfur becomes a negatively charged ion (S²⁻) and the metal becomes a positively charged ion (Na⁺). These oppositely charged ions attract each other, forming an ionic bond.
In short, sulfur gains electrons in ionic bonds to achieve a stable octet configuration and a negative charge.
