The molecule C₃H₄ is an unsaturated hydrocarbon, which means it contains carbon-carbon double or triple bonds. To determine its Lewis structure, we'll consider the valence electrons of carbon and hydrogen.

Step 1: Count the Total Valence Electrons for C₃H₄:

Carbon (C) has 4 valence electrons.
Hydrogen (H) has 1 valence electron.

Total valence electrons from carbon: 3 × 4 = 12 electrons
Total valence electrons from hydrogen: 4 × 1 = 4 electrons
Combined, C₃H₄ has 16 valence electrons.

Step 2: Determine the Central Atoms

Carbon atoms will serve as the backbone of the molecule. The hydrogens will attach to the carbons.

Step 3: Place the Atoms and Start with Single Bonds

Place the three carbon atoms in a row and connect them with single bonds. Attach the hydrogen atoms to the carbon atoms. There are formed two possible structures:

Step 4: Complete the Octet for Each Carbon

Each carbon atom needs 8 electrons to complete its octet.

In structure A: The middle carbon atom will form a triple bond with one of the other carbon atoms, while the third carbon atom will form single bonds with the remaining hydrogens.

In structure B: The middle carbon atom will form two double bonds with both lateral carbon atoms, which on the other hand will form single bonds with the remaining hydrogens.

Step 5: Verify the Structure

Ensure that each carbon atom has a complete octet (or 4 bonds in the case of carbon) and each hydrogen atom is connected by a single bond.

The Lewis structures for C₃H₄ can be represented as:

c3h4 lewis structures

The Lewis structures for C3​H4​ can be represented as:

The Lewis structures for C₃H₄ can be represented as:

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