In the reaction `3Mg+N_(2)rarrMg_(3)N_(2)`

Options

A. Magnesium is reduced
B. Magnesium is oxidized
C. Nitrogen is oxidized
D. Nitrogen is reduced

Explanation

To analyze the redox reaction \(3Mg + N_2 \rightarrow Mg_3N_2\), we need to determine the oxidation states of the elements involved and identify which ones are oxidized and reduced.

### Step 1: Determine the oxidation states of the reactants
- In the reaction, magnesium (Mg) is in its elemental form, so its oxidation state is 0.
- Nitrogen (N) is also in its elemental form as \(N_2\), so its oxidation state is also 0.

### Step 2: Determine the oxidation states in the product \(Mg_3N_2\)
- Let the oxidation state of magnesium in \(Mg_3N_2\) be \(+x\). Since there are 3 magnesium atoms, the total contribution from magnesium is \(3x\).
- The oxidation state of nitrogen in \(Mg_3N_2\) is typically \(-3\) (as it usually has a -3 oxidation state in nitrides).
- The compound is neutral, so the sum of the oxidation states must equal 0:
\[ 3x + 2(-3) = 0 \]
Simplifying this gives:
\[ 3x - 6 = 0 \implies 3x = 6 \implies x = +2 \]
- Therefore, the oxidation state of magnesium in \(Mg_3N_2\) is \(+2\), and the oxidation state of nitrogen is \(-3\).

### Step 3: Identify oxidation and reduction
- **Oxidation** is defined as an increase in oxidation state, while **reduction** is a decrease in oxidation state.
- Magnesium changes from an oxidation state of 0 to +2, indicating that it is oxidized.
- Nitrogen changes from an oxidation state of 0 to -3, indicating that it is reduced.

### Conclusion
- Magnesium is oxidized (oxidation state increases from 0 to +2).
- Nitrogen is reduced (oxidation state decreases from 0 to -3).

### Final Answer:
- Magnesium is oxidized.
- Nitrogen is reduced.