Assertion: The bond energy of `gt C = O` is less than `gt C = C lt` in alkenes.
Reason: The carbon atom in carbonyl group is `sp^(2)` hybridised.

Options

A. If both assertion and reason are true and the reason is the correct explanation of the assertion
B. If both assertion and reason are true but reason is not the correct explanation of the assertion
C. If assertion is true but reason is false
D. If assertion is false but reason is true

Explanation

To analyze the assertion and reason provided in the question, we can break it down into a step-by-step solution.

### Step 1: Understand the Assertion
The assertion states that the bond energy of the carbon-oxygen double bond (C=O) is less than that of the carbon-carbon double bond (C=C) in alkenes.

### Step 2: Evaluate the Bond Energies
- **C=C Bond**: The bond energy of a carbon-carbon double bond is relatively high due to the strong overlap of the p-orbitals involved in the π-bond formation.
- **C=O Bond**: The carbon-oxygen double bond has a significant amount of double bond character, but it is also influenced by the electronegativity difference between carbon and oxygen, which can lead to polarization.
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