`3Mg(s)+N_(2)(g)overset(Delta)toMg_(3)N_(2)`

Options

A. For disproportionation reaction.
B. For comproportionation reaction.
C. For either intermolecular redox reaction or displacement reaction
D. For either thermal combination redox reaction or thermal decomposition redox reaction.

Answer

To analyze the given reaction \(3Mg(s) + N_2(g) \overset{\Delta}{\rightarrow} Mg_3N_2\), we will determine the type of reaction it represents.

### Step-by-Step Solution:

**Step 1: Identify the reactants and products.**
- The reactants are magnesium (Mg) in solid form and nitrogen (N₂) in gaseous form.
- The product is magnesium nitride (Mg₃N₂).

**Step 2: Determine the nature of the reaction.**
- This reaction involves the combination of two elements (magnesium and nitrogen) to form a single compound (magnesium nitride).

**Step 3: Classify the reaction.**
- A reaction where two or more reactants combine to form a single product is known as a combination reaction.
- In this case, since magnesium and nitrogen are combining to form magnesium nitride, it fits the definition of a combination reaction.

**Step 4: Check for other reaction types.**
- **Disproportionation Reaction:** This does not apply here as there is no element being simultaneously oxidized and reduced.
- **Comproportionation Reaction:** This does not apply as there are no elements in different oxidation states combining to form an intermediate state.
- **Displacement Reaction:** This does not apply as there is no replacement of an ion in a compound.
- **Decomposition Reaction:** This does not apply as the reactants are not breaking down into simpler products.

**Conclusion:**
- The reaction \(3Mg(s) + N_2(g) \overset{\Delta}{\rightarrow} Mg_3N_2\) is a **combination reaction**.

### Final Answer:
The correct classification for the reaction is a **combination reaction**.

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