Assertion (A) The `alpha`-hydrogen atom in carbonyl compounds is less acidic.
Reason (R) The anion formed after the loss of `alpha`-hydrogen atom is resonance stabilised.

Explanation

To analyze the assertion and reason provided in the question, we can break down the concepts step by step.

### Step 1: Understand the Assertion
The assertion states that "the alpha-hydrogen atom in carbonyl compounds is less acidic." This means that the alpha-hydrogen is not likely to donate a proton (H⁺) easily.

**Hint:** Remember that acidity is determined by how easily a hydrogen atom can be removed as a proton.

### Step 2: Analyze the Reason
The reason given is that "the anion formed after the loss of alpha-hydrogen atom is resonance stabilized." This implies that when the alpha-hydrogen is removed, the resulting anion (conjugate base) is stabilized by resonance.

**Hint:** Consider how resonance stabilization affects the stability of anions and their propensity to form.

### Step 3: Evaluate the Acidity of Alpha-Hydrogens
In carbonyl compounds (like aldehydes and ketones), the alpha-hydrogens are indeed acidic. When a strong base is introduced, it can abstract the alpha-hydrogen, leading to the formation of a resonance-stabilized anion. This stabilization makes the loss of the alpha-hydrogen more favorable, indicating that the alpha-hydrogens are, in fact, more acidic.

**Hint:** Think about the stability of the conjugate base formed after deprotonation and how resonance contributes to that stability.

### Step 4: Conclusion
Based on the analysis:
- The assertion is incorrect because alpha-hydrogens in carbonyl compounds are more acidic, not less.
- The reason is correct because the anion formed after the loss of alpha-hydrogen is indeed resonance stabilized.

Thus, the correct conclusion is that the assertion is false, while the reason is true.

**Final Answer:** The assertion (A) is incorrect, and the reason (R) is correct. Therefore, the correct option is that the assertion is wrong, but the reason is correct.