`3Mg(s)+N_(2)(g)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 reaction \(3Mg(s) + N_2(g) \rightarrow Mg_3N_2\), we will break it down step by step.

### Step 1: Identify the Reactants and Products
The reactants in this reaction are magnesium (Mg) in solid form and nitrogen (N₂) in gaseous form. The product formed is magnesium nitride (Mg₃N₂).

### Step 2: Determine the Oxidation States
- In elemental form, magnesium (Mg) has an oxidation state of 0.
- In nitrogen (N₂), nitrogen also has an oxidation state of 0.
- In magnesium nitride (Mg₃N₂), magnesium has an oxidation state of +2, and nitrogen has an oxidation state of -3.

### Step 3: Analyze the Changes in Oxidation States
- Magnesium (Mg) changes from 0 to +2, indicating that it is **oxidized** (loss of electrons).
- Nitrogen (N₂) changes from 0 to -3, indicating that it is **reduced** (gain of electrons).

### Step 4: Classify the Reaction
Now that we have established that one element is oxidized and the other is reduced, we can classify the type of reaction:
- This reaction involves the combination of two elements (Mg and N₂) to form a compound (Mg₃N₂).
- Since heat is required for this reaction to occur, it is also classified as a **thermal reaction**.

### Step 5: Conclusion
The reaction \(3Mg(s) + N_2(g) \rightarrow Mg_3N_2\) is a **thermal combination redox reaction** because:
- It is a combination reaction (two reactants combine to form one product).
- It involves oxidation and reduction (redox).
- It requires heat for the reaction to proceed.

### Final Answer
The correct classification of the reaction is a **thermal combination redox reaction**.

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