Assertion `F_(2)` does not undrego disporportionation reaction
Reason Fluorine shows only 0 and -1 oxidation states

Options

A. If both assertion and reasn are true and reason is the true explanation of the assertion
B. If both assertion and reason are true but reason is not the true explanation of the assertion
C. If assertion is true but reason is false
D. If both assertion and reason are false

Explanation

To analyze the assertion and reason provided in the question, we will break down the concepts step by step.

### Step 1: Understand the Assertion
The assertion states that \( F_2 \) does not undergo a disproportionation reaction. A disproportionation reaction is a type of redox reaction where a single substance is both oxidized and reduced, resulting in two different products.

**Hint:** Consider what it means for a substance to be both oxidized and reduced in a reaction.

### Step 2: Understand the Reason
The reason given is that fluorine shows only 0 and -1 oxidation states. In its elemental form \( F_2 \), fluorine has an oxidation state of 0. When fluorine forms compounds, it typically exhibits an oxidation state of -1 (as in \( HF \)).

**Hint:** Recall the common oxidation states of fluorine and how they relate to its reactivity.

### Step 3: Analyze Oxidation States
Fluorine, being the most electronegative element, can only exist in the -1 oxidation state when it is in a compound. It does not exhibit positive oxidation states because it cannot lose electrons; it always tends to gain them.

**Hint:** Think about why electronegativity affects oxidation states and the ability to undergo oxidation.

### Step 4: Connection to Disproportionation
Since \( F_2 \) can only exist in the oxidation states of 0 (in \( F_2 \)) and -1 (in compounds), it cannot be oxidized to a positive oxidation state. For a disproportionation reaction to occur, there must be a species that can be oxidized (increase in oxidation state) and reduced (decrease in oxidation state). Since fluorine cannot be oxidized to a positive state, it cannot undergo disproportionation.

**Hint:** Reflect on the requirements for a substance to participate in a disproportionation reaction.

### Step 5: Conclusion
Thus, the assertion is true: \( F_2 \) does not undergo disproportionation reactions. The reason is also true: fluorine shows only 0 and -1 oxidation states. However, while both statements are true, the reason does not correctly explain why the assertion is true. Therefore, the assertion is true, but the reason is not a correct explanation of the assertion.

### Final Answer
- Assertion: True
- Reason: True, but does not correctly explain the assertion.