How do you draw the Lewis structure of SF₆?

SF₆ has 48 valence electrons. Sulfur forms 6 single bonds to fluorine, using 12 electrons; 36 remain. Each F gets 3 lone pairs (6 electrons x 6 = 36). All 36 remaining electrons accounted for.

Lewis Structure of SF₆ (Sulfur Hexafluoride)

What is the Lewis structure of SF₆?

SF₆ has 48 valence electrons, 6 bonding electron pairs, and 18 lone pairs. SF₆ has 48 valence electrons. Twelve are in six S-F single bonds, and 36 form 3 lone pairs on each fluorine. Sulfur has 12 electrons around it, well beyond the octet. This is possible because S uses 3d orbitals. The geometry is octahedral and the molecule is nonpolar despite the polar S-F bonds.

Lewis structure of SF₆ (Sulfur Hexafluoride)

Formula	SF₆
Name	Sulfur Hexafluoride
Total Valence Electrons	48
Lone Pairs	18
Has Resonance	No
Concept	Expanded Octet
Difficulty	Advanced

Step 1: Count Valence Electrons

S has 6, each F has 7: 6 + 6(7) = 48 total.

Step 2: Draw the Skeleton

Sulfur forms 6 single bonds to fluorine, using 12 electrons; 36 remain.

Step 3: Distribute Lone Pairs

Each F gets 3 lone pairs (6 electrons x 6 = 36). All 36 remaining electrons accounted for.

Step 4: Form Multiple Bonds

No multiple bonds needed. S has 12 electrons from 6 bonds. This is one of the most well-known examples of an expanded octet.

Step 5: Check Formal Charges

S: FC = 6 - 0 - ½(12) = 0
F: FC = 7 - 6 - ½(2) = 0
All formal charges are zero despite S having 12 electrons.

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