How do you draw the Lewis structure of PO₄³⁻?

Q: How do you draw the Lewis structure of PO₄³⁻?

PO₄³⁻ has 32 valence electrons. Phosphorus is central, bonded to four oxygens. Four single bonds use 8 electrons; 24 remain. Each O gets 3 lone pairs (24 electrons total). P has a full octet from 4 bonds.

Lewis Structure of PO₄³⁻ (Phosphate)

What is the Lewis structure of PO₄³⁻?

PO₄³⁻ has 32 valence electrons, 4 bonding electron pairs, and 12 lone pairs. PO₄³⁻ has 32 valence electrons. Eight are in four P-O single bonds, and 24 form 3 lone pairs on each oxygen. Phosphorus has FC = +1 and each oxygen has FC = -1, giving a net charge of -3.

Lewis structure of PO₄³⁻ (Phosphate)

Formula	PO₄³⁻
Name	Phosphate
Total Valence Electrons	32
Lone Pairs	12
Has Resonance	No
Concept	Polyatomic Ion
Difficulty	Advanced

Step 1: Count Valence Electrons

P has 5, each O has 6, plus 3 for the charge: 5 + 4(6) + 3 = 32.

Step 2: Draw the Skeleton

Phosphorus is central, bonded to four oxygens. Four single bonds use 8 electrons; 24 remain.

Step 3: Distribute Lone Pairs

Each O gets 3 lone pairs (24 electrons total). P has a full octet from 4 bonds.

Step 4: Form Multiple Bonds

No multiple bonds in the octet-following structure. Expanded octet versions with P=O double bonds are sometimes drawn.

Step 5: Check Formal Charges

P: FC = 5 - 0 - ½(8) = +1
O: FC = 6 - 6 - ½(2) = -1 (each)
Net: +1 + 4(-1) = -3, matching the ion charge.

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