Question

which of the following correctly compares the strength of the two carbon-to-carbon bonds in the molecule represented in the lewis diagram shown above? a the carbon-to-carbon bond on the left is stronger because it is a double bond. b the carbon-to-carbon bonds are the same strength because the c-c-c bond angle is 180°. c the carbon-to-carbon bonds are the same strength because they are both bonds between carbon atoms. d the carbon-to-carbon bond on the right is stronger because there are more hydrogen atoms attached to the rightmost carbon atom than to the leftmost carbon atom.

Explanation:

To solve this, we analyze each option:

• Option A: Double bonds (C=C) are stronger than single bonds (C - C) because a double bond has a sigma and a pi bond, while a single bond has only a sigma bond. The left bond is a double bond, so it's stronger.
• Option B: Bond angle (180° here, due to sp² and sp³ hybridization) doesn't determine bond strength. Bond strength depends on bond type (single, double, triple), so this is wrong.
• Option C: Just being C - C bonds doesn't mean same strength. Double and single C - C bonds differ in strength, so this is wrong.
• Option D: Number of H atoms attached doesn't affect C - C bond strength. Bond strength is about the bond between C atoms, not substituents, so this is wrong.

Answer:

A. The carbon - to - carbon bond on the left is stronger because it is a double bond.