Assertion (A) The O-O bond length in `H_(2)O_(2)` is shorter than that in `O_(2)`.
Reason (R ) `H_(2)O_(2)` is ionic compound.

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.

Explanation

To solve the given question, we need to analyze both the assertion (A) and the reason (R) provided. Let's break down the solution step by step.

### Step 1: Analyze the Assertion (A)
The assertion states that the O-O bond length in H₂O₂ (hydrogen peroxide) is shorter than that in O₂ (dioxygen).

1. **Understanding the Structures**:
- **H₂O₂** has an open book structure with the formula H-O-O-H. The bond between the two oxygen atoms is a single bond.
- **O₂** consists of two oxygen atoms connected by a double bond (O=O).

2. **Bond Order**:
- The bond order of the O-O bond in H₂O₂ is 1 (single bond).
- The bond order of the O-O bond in O₂ is 2 (double bond).

3. **Relationship Between Bond Order and Bond Length**:
- Generally, a higher bond order corresponds to a shorter bond length. Therefore, since O₂ has a higher bond order than H₂O₂, it will have a shorter bond length.

4. **Conclusion for Assertion**:
- Since the bond length in H₂O₂ is actually longer than in O₂, the assertion (A) is **false**.

### Step 2: Analyze the Reason (R)
The reason states that H₂O₂ is an ionic compound.

1. **Nature of H₂O₂**:
- H₂O₂ is not an ionic compound; it is a polar covalent compound. This is due to the difference in electronegativity between hydrogen and oxygen, which leads to a polar covalent bond.

2. **Conclusion for Reason**:
- Since H₂O₂ is not ionic but rather polar covalent, the reason (R) is also **false**.

### Final Conclusion
Both the assertion (A) and the reason (R) are false. Therefore, the correct answer is option D: both A and R are false.

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