How do you draw the Lewis structure of CO?

CO has 10 valence electrons. Start with a single bond (2 electrons). 8 remain. After forming the triple bond, each atom has 1 lone pair (2 electrons).

Lewis Structure of CO (Carbon Monoxide)

What is the Lewis structure of CO?

CO has 10 valence electrons, 3 bonding electron pairs, and 2 lone pairs. CO has 10 valence electrons. Six are shared in a C-O triple bond, and each atom has one lone pair. Unusually, carbon has a formal charge of -1 and oxygen has +1, making CO a strong ligand in coordination chemistry.

Lewis structure of CO (Carbon Monoxide)

Formula	CO
Name	Carbon Monoxide
Total Valence Electrons	10
Lone Pairs	2
Has Resonance	No
Concept	Multiple Bonds
Difficulty	Intermediate

Step 1: Count Valence Electrons

C has 4, O has 6: 4 + 6 = 10 total valence electrons.

Step 2: Draw the Skeleton

Start with a single bond (2 electrons). 8 remain.

Step 3: Distribute Lone Pairs

After forming the triple bond, each atom has 1 lone pair (2 electrons).

Step 4: Form Multiple Bonds

Convert lone pairs into bonding pairs until both atoms have octets: single to triple bond (C≡O). Each atom: 6 bonding + 2 lone pair = 8 electrons.

Step 5: Check Formal Charges

C: FC = 4 - 2 - ½(6) = -1
O: FC = 6 - 2 - ½(6) = +1
The negative charge on C (more electropositive atom) is counterintuitive but correct.

Interactive Lewis structure builder with guided walkthroughs and practice quizzes.

Build the CO Lewis Structure Step by Step