Statement-1 : `H_(2)O` is liquid whereas `H_(2)S` is gas .
and
Statement-2 : Oxygen is more electronegative than sulphur .

Options

A. (A) Statement-1 is True , Statement-2 is True , Statement-2 is a correct explanation for Statement-1
B. (B) Statement-1 is True , Statement-2 is True , Statement-2 is NOT a correct explanation for Statement-1
C. (C) Statement-1 is True , Statement-2 is False
D. (D) Statement-1 is False , Statement-2 is True

Answer

To analyze the statements given in the question, we will break down the reasoning step by step.

### Step 1: Analyze Statement 1
- **Statement 1**: `H2O` is liquid whereas `H2S` is gas.
- **Explanation**: Water (`H2O`) exists in the liquid state at room temperature, while hydrogen sulfide (`H2S`) is a gas. The primary reason for this difference is the presence of hydrogen bonding in water. In `H2O`, the highly electronegative oxygen atom forms hydrogen bonds with the hydrogen atoms, leading to a more compact and stable liquid structure. In contrast, `H2S` does not form hydrogen bonds because sulfur is less electronegative than oxygen, resulting in weaker intermolecular forces and allowing `H2S` to exist as a gas.

### Step 2: Analyze Statement 2
- **Statement 2**: Oxygen is more electronegative than sulfur.
- **Explanation**: This statement is true. Electronegativity is a measure of an atom's ability to attract electrons in a bond. Oxygen is located above sulfur in the periodic table, and as we move down a group, electronegativity decreases due to the increase in atomic size and the distance of the valence electrons from the nucleus. Therefore, oxygen, being smaller and having a higher effective nuclear charge, is more electronegative than sulfur.

### Step 3: Determine the Relationship Between the Statements
- **Explanation**: While both statements are true, Statement 2 does not directly explain why `H2O` is a liquid and `H2S` is a gas. The reason for the difference in states of matter is primarily due to the hydrogen bonding in `H2O`, which is a consequence of oxygen's higher electronegativity. However, the statement about electronegativity alone does not address the presence or absence of hydrogen bonding in these compounds.

### Conclusion
- **Final Assessment**:
- Statement 1 is true.
- Statement 2 is true.
- Statement 2 is not a correct explanation for Statement 1.

### Answer Options
- The correct option is: **Statement 1 is true and Statement 2 is true, but Statement 2 is not a correct explanation for Statement 1**.

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