Uploaded April 2025 | Updated September 2026, 2 weeks ago
How to Draw the Lewis Structure for SO₂ (Sulfur Dioxide)
In this video, we go step-by-step through how to draw the Lewis structure for SO₂ and explain the reasoning behind each move.
Step 1: Count the valence electrons.
We begin by adding up the valence electrons: sulfur has 6, and each oxygen has 6, for a total of 18 valence electrons.
Step 2: Choose a central atom.
Sulfur is the least electronegative (excluding hydrogen, which isn't here), so we place it at the center.
Step 3: Create single bonds and distribute electrons.
We form single bonds between sulfur and the two oxygens, then distribute the remaining electrons to satisfy octets.
Step 4: Check for octets.
After placing lone pairs, we see that sulfur doesn’t have a full octet. We adjust by creating double bonds.
Step 5: Evaluate formal charges.
Even though one structure satisfies the octet rule, it carries non-zero formal charges. By forming a second double bond, we create a structure where all atoms have octets and formal charges are minimized — this is the most stable Lewis structure.
📌 Note: While this is the best single drawing, SO₂ is actually a resonance hybrid of multiple structures. See the pinned comment below for more detail.
• Lewis Structures Made Simple: • How to Draw Lewis Structures: Five Ea...
• More practice: • Lewis Dot Structure Practice Problems...
• Counting Valence Electrons: • Finding the Number of Valence Electro...
• Calculating Formal Charge: • Formal Charges: Calculating Formal Ch...
• Exceptions to the Octet Rule: • Exceptions to the Octet Rule
How to Draw the Lewis Structure for SO₂ (Sulfur Dioxide)
In this video, we go step-by-step through how to draw the Lewis structure for SO₂ and explain the reasoning behind each move.
Step 1: Count the valence electrons.
We begin by adding up the valence electrons: sulfur has 6, and each oxygen has 6, for a total of 18 valence electrons.
Step 2: Choose a central atom.
Sulfur is the least electronegative (excluding hydrogen, which isn't here), so we place it at the center.
Step 3: Create single bonds and distribute electrons.
We form single bonds between sulfur and the two oxygens, then distribute the remaining electrons to satisfy octets.
Step 4: Check for octets.
After placing lone pairs, we see that sulfur doesn’t have a full octet. We adjust by creating double bonds.
Step 5: Evaluate formal charges.
Even though one structure satisfies the octet rule, it carries non-zero formal charges. By forming a second double bond, we create a structure where all atoms have octets and formal charges are minimized — this is the most stable Lewis structure.
📌 Note: While this is the best single drawing, SO₂ is actually a resonance hybrid of multiple structures. See the pinned comment below for more detail.
• Lewis Structures Made Simple: • How to Draw Lewis Structures: Five Ea...
• More practice: • Lewis Dot Structure Practice Problems...
• Counting Valence Electrons: • Finding the Number of Valence Electro...
• Calculating Formal Charge: • Formal Charges: Calculating Formal Ch...
• Exceptions to the Octet Rule: • Exceptions to the Octet Rule
