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 determine whether lithium or nitrogen is being oxidized or reduced in the reaction \(6Li + N_2 \rightarrow 2Li_3N\), we can analyze the changes in oxidation states of the elements involved.

### Step-by-Step Solution:

1. **Identify the Reactants and Products:**
- Reactants: Lithium (Li) and Nitrogen (\(N_2\))
- Product: Lithium nitride (\(Li_3N\))

2. **Determine the Oxidation States:**
- In the elemental form, the oxidation state of lithium (Li) is 0.
- In \(N_2\), the oxidation state of nitrogen is also 0.
- In lithium nitride (\(Li_3N\)):
- Let the oxidation state of lithium be \(x\).
- The compound is neutral, so:
\[ 3x + (-3) = 0 \implies 3x = 3 \implies x = +1 \]
- Therefore, the oxidation state of lithium in \(Li_3N\) is +1, and the oxidation state of nitrogen is -3.

3. **Analyze the Changes in Oxidation States:**
- Lithium changes from 0 to +1 (oxidation).
- Nitrogen changes from 0 to -3 (reduction).

4. **Conclusion:**
- Since lithium's oxidation state increases, it is being oxidized.
- Since nitrogen's oxidation state decreases, it is being reduced.

### Final Answer:
- Lithium is being oxidized, and nitrogen is being reduced in the reaction.