Assertion :- In `HClO_(4)`, Chlorine has the oxidation number of `+4`.
Reason :- `HClO_(4)` (perchloric) acid has two peroxide linkage.

Options

A. If both Assertion & Reason are True & the Reason is a correct explanation of the Assertion.
B. If both Assertion & Reason are True but Reason is not a correct explanation of the Assertion.
C. If Assertion is True but the Reason is False.
D. If both Assertion & Reason are False.

Answer

To solve the question, we need to analyze the assertion and the reason provided regarding the oxidation state of chlorine in perchloric acid (HClO₄) and the presence of peroxide linkages.

### Step-by-Step Solution:

1. **Identify the Compound**: We start with the compound HClO₄, which is known as perchloric acid.

2. **Determine the Oxidation State of Chlorine**:
- The oxidation state of hydrogen (H) is +1.
- The oxidation state of oxygen (O) is typically -2.
- Let the oxidation state of chlorine (Cl) be denoted as X.

3. **Set Up the Equation**:
- The formula for the compound is HClO₄. The total charge of the molecule is 0 (neutral compound).
- The equation based on the oxidation states is:
\[ X + 1 + 4(-2) = 0 \]
- Simplifying this gives:
\[ X + 1 - 8 = 0 \]
\[ X - 7 = 0 \]
\[ X = +7 \]

4. **Conclusion on the Assertion**:
- The assertion states that the oxidation number of chlorine in HClO₄ is +4. However, we calculated it to be +7. Therefore, the assertion is **false**.

5. **Analyze the Reason**:
- The reason states that HClO₄ has two peroxide linkages. A peroxide linkage typically involves an O-O bond, which is not present in HClO₄.
- In HClO₄, the structure consists of three double-bonded oxygens and one hydroxyl group (OH), with no O-O bonds.
- Therefore, the reason is also **false**.

6. **Final Conclusion**:
- Since both the assertion and the reason are false, the correct answer is that both are incorrect.

### Final Answer:
Both the assertion and the reason are false.

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