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 and the reason is the correct explanation of the assertion, then mark (1)
B. If both Assertion & Reason are true but the reason is not the correct explanantion of the assertion, then mark (2)
C. If assertion is true statements but Reason is false, then mark (3)
D. If both Assertion and Reason are false statements, then mark (4)

Answer

To solve the question, we need to analyze both the assertion and the reason provided.

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

- **Bond Length Comparison**:
- In O₂, the bond between the two oxygen atoms is a double bond (O=O), which typically results in a shorter bond length due to the stronger attraction between the atoms.
- In H₂O₂, the bond between the two oxygen atoms is a single bond (O-O), which is longer than a double bond.

**Conclusion for Assertion**: The assertion is **false** because the O-O bond length in H₂O₂ is longer than that in O₂.

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

- **Nature of H₂O₂**:
- Hydrogen peroxide is not an ionic compound; it is a polar covalent compound. This is due to the presence of covalent bonds between hydrogen and oxygen atoms, and the molecule has a dipole moment because of the difference in electronegativity between hydrogen and oxygen.

**Conclusion for Reason**: The reason is also **false** because H₂O₂ is not an ionic compound.

### Final Conclusion
Both the assertion and the reason are false. Therefore, the correct answer is that both the assertion and the reason are false.

### Summary of the Solution:
1. The assertion about the bond length in H₂O₂ being shorter than in O₂ is false.
2. The reason stating that H₂O₂ is an ionic compound is also false.
3. Thus, both the assertion and reason are false.