Assertion: `Na_(2)O_(2)` is coloured and paramagnetic
Reason: `Na_(2)O_(2)` is superoxide

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 question, we need to analyze the assertion and the reason provided regarding sodium peroxide (\(Na_2O_2\)).

### Step 1: Determine the oxidation state of oxygen in \(Na_2O_2\)
- We know that sodium (\(Na\)) is an alkali metal and has an oxidation state of +1.
- The formula for sodium peroxide is \(Na_2O_2\). Let the oxidation state of oxygen be \(x\).
- The equation can be set up as follows:
\[ 2(+1) + 2x = 0 \]
Simplifying this gives:
\[ 2 + 2x = 0 \implies 2x = -2 \implies x = -1 \]
- Therefore, the oxidation state of oxygen in \(Na_2O_2\) is -1.

### Step 2: Identify the nature of \(Na_2O_2\)
- Since the oxidation state of oxygen is -1, \(Na_2O_2\) is classified as a peroxide.
- Peroxides typically contain the \(O_2^{2-}\) ion, which does not have unpaired electrons.

### Step 3: Analyze the assertion and reason
- The assertion states that \(Na_2O_2\) is colored and paramagnetic.
- The reason states that \(Na_2O_2\) is a superoxide.
- However, we have established that \(Na_2O_2\) is a peroxide, not a superoxide. Superoxides contain the \(O_2^{-}\) ion and have different properties.

### Step 4: Determine the magnetic properties
- Since \(Na_2O_2\) is a peroxide, it has no unpaired electrons (as established earlier).
- Compounds with no unpaired electrons are diamagnetic and typically colorless.

### Conclusion
- Both the assertion (that \(Na_2O_2\) is colored and paramagnetic) and the reason (that \(Na_2O_2\) is a superoxide) are incorrect.
- Therefore, the correct answer is that both the assertion and reason are false.

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

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