How do you draw the Lewis structure of PCl₅?

PCl₅ has 40 valence electrons. Phosphorus forms 5 single bonds to chlorine, using 10 electrons; 30 remain. Each Cl gets 3 lone pairs (6 electrons), using all 30 remaining electrons.

Lewis Structure of PCl₅ (Phosphorus Pentachloride)

What is the Lewis structure of PCl₅?

PCl₅ has 40 valence electrons, 5 bonding electron pairs, and 15 lone pairs. PCl₅ has 40 valence electrons. Five P-Cl single bonds use 10 electrons, and each Cl has 3 lone pairs (30 electrons). Phosphorus has 10 electrons around it, exceeding the octet. This is possible because P is in Period 3 and can use d orbitals. The geometry is trigonal bipyramidal.

Lewis structure of PCl₅ (Phosphorus Pentachloride)

Formula	PCl₅
Name	Phosphorus Pentachloride
Total Valence Electrons	40
Lone Pairs	15
Has Resonance	No
Concept	Expanded Octet
Difficulty	Advanced

Step 1: Count Valence Electrons

P has 5, each Cl has 7: 5 + 5(7) = 40 total.

Step 2: Draw the Skeleton

Phosphorus forms 5 single bonds to chlorine, using 10 electrons; 30 remain.

Step 3: Distribute Lone Pairs

Each Cl gets 3 lone pairs (6 electrons), using all 30 remaining electrons.

Step 4: Form Multiple Bonds

No multiple bonds needed. P has 10 electrons around it (5 bonds). This is an expanded octet, allowed for elements in Period 3 and beyond that can access d orbitals.

Step 5: Check Formal Charges

P: FC = 5 - 0 - ½(10) = 0
Cl: FC = 7 - 6 - ½(2) = 0
Despite the expanded octet, all formal charges are zero.

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