Assertion : H-S-H bond angle in `H_(2)S` is closer to `90^(@)` but H-O-H bond angle in `H_(2)O` is `104.5^(@)`
Reason: lp-lp repulsion is stronger in `H_(2)S` than in `H_(2)O`

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 the assertion and reason both are false

Explanation

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

### Step 1: Understanding the Assertion
The assertion states that the H-S-H bond angle in H₂S is closer to 90 degrees, while the H-O-H bond angle in H₂O is 104.5 degrees.

**Hint:** Consider the molecular geometry and hybridization of both molecules.

### Step 2: Molecular Geometry of H₂S and H₂O
H₂S has a bent molecular geometry due to the presence of two lone pairs on the sulfur atom. H₂O also has a bent geometry but with two lone pairs on the oxygen atom.

**Hint:** Recall the VSEPR theory to determine the shape based on lone pairs and bond pairs.

### Step 3: Electronegativity and Bond Pair Repulsion
The electronegativity of oxygen is higher than that of sulfur. This means that in H₂O, the bond pairs (O-H) are pulled closer to the oxygen, increasing the repulsion between the bond pairs.

**Hint:** Compare the electronegativities of sulfur and oxygen to understand their effect on bond angles.

### Step 4: Lone Pair Repulsion
In H₂O, the lone pairs are more repulsive due to the higher electronegativity of oxygen, which leads to a greater angle between the H-O-H bonds. In contrast, in H₂S, the lower electronegativity of sulfur means that the bond pairs are less repelled, resulting in a smaller angle closer to 90 degrees.

**Hint:** Think about how lone pairs affect the bond angles in different molecules.

### Step 5: Evaluating the Reason
The reason states that lone pair-lone pair repulsion is stronger in H₂S than in H₂O. This is incorrect because the lone pair-lone pair repulsion is actually stronger in H₂O due to the higher electronegativity of oxygen.

**Hint:** Analyze the relationship between electronegativity and lone pair repulsion in both molecules.

### Conclusion
Both the assertion and reason are true statements, but the reason provided does not correctly explain the assertion. Therefore, the correct conclusion is that the assertion is true, but the reason is false.

**Final Answer:** The assertion is true, but the reason is false.