In the reaction `6Li+N_(2)rarr2Li_(3)N`

Options

A. Li undergoes reduction
B. Li undergoes oxidation
C. N undergoes oxidation
D. None of these

Answer

To solve the question regarding the reaction \(6 \text{Li} + \text{N}_2 \rightarrow 2 \text{Li}_3\text{N}\), we need to analyze the oxidation states of the elements involved and determine the changes that occur during the reaction.

### Step-by-Step Solution:

1. **Identify the Reactants and Products:**
- Reactants: Lithium (Li) and Nitrogen (N2)
- Products: Lithium Nitride (Li3N)

2. **Determine the Oxidation States:**
- In elemental form, the oxidation state of lithium (Li) is 0.
- In molecular nitrogen (N2), the oxidation state of nitrogen is also 0.
- In lithium nitride (Li3N), lithium has an oxidation state of +1 (since it is an alkali metal) and nitrogen has an oxidation state of -3.

3. **Calculate the Change in Oxidation States:**
- For lithium:
- Initial oxidation state = 0 (in Li)
- Final oxidation state = +1 (in Li3N)
- Change = +1 - 0 = +1 (oxidation)
- For nitrogen:
- Initial oxidation state = 0 (in N2)
- Final oxidation state = -3 (in Li3N)
- Change = -3 - 0 = -3 (reduction)

4. **Identify the Oxidation and Reduction:**
- Lithium is oxidized (loses electrons) as its oxidation state increases from 0 to +1.
- Nitrogen is reduced (gains electrons) as its oxidation state decreases from 0 to -3.

5. **Conclusion:**
- Since lithium undergoes oxidation, the correct answer is that lithium is oxidized in this reaction.

### Final Answer:
- The correct option is **B**: Lithium undergoes oxidation.