`Ba(N_(3))_(2) overset(Delta) to Ba+N_(2)uarr`

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 solve the given question regarding the reaction \( \text{Ba(N}_3\text{)}_2 \overset{\Delta}{\rightarrow} \text{Ba} + \text{N}_2 \), we will analyze the reaction step by step.

### Step 1: Identify the Reactants and Products
The reactant is barium azide, \( \text{Ba(N}_3\text{)}_2 \), and the products are barium (\( \text{Ba} \)) and nitrogen gas (\( \text{N}_2 \)).

**Hint:** Look at the chemical formula to identify the elements involved in the reaction.

### Step 2: Determine Oxidation States
- For barium in \( \text{Ba(N}_3\text{)}_2 \), the oxidation state is +2 (since barium typically has a +2 oxidation state).
- For nitrogen in \( \text{Ba(N}_3\text{)}_2 \), let’s calculate the oxidation state. The total charge must equal zero:
\[ +2 + 3x = 0 \quad \Rightarrow \quad 3x = -2 \quad \Rightarrow \quad x = -\frac{2}{3} \]
Thus, the oxidation state of nitrogen in \( \text{Ba(N}_3\text{)}_2 \) is \(-\frac{2}{3}\).

**Hint:** Use the charge balance to find the oxidation states of elements in compounds.

### Step 3: Analyze the Products
- In the products, barium (\( \text{Ba} \)) is in the elemental state, so its oxidation state is 0.
- Nitrogen gas (\( \text{N}_2 \)) also has an oxidation state of 0.

**Hint:** Remember that elements in their elemental form have an oxidation state of zero.

### Step 4: Identify Changes in Oxidation States
- Barium changes from +2 to 0 (reduction).
- Nitrogen changes from \(-\frac{2}{3}\) to 0 (oxidation).

**Hint:** Compare the oxidation states of reactants and products to determine which elements are oxidized and reduced.

### Step 5: Classify the Reaction
Since barium is reduced and nitrogen is oxidized, this is a redox reaction. Additionally, since a single reactant decomposes into two products, it is classified as a decomposition reaction. Specifically, since heat is applied (indicated by \( \Delta \)), it is a thermal decomposition reaction.

**Hint:** A reaction that involves the breakdown of a single compound into two or more products is a decomposition reaction.

### Conclusion
The reaction \( \text{Ba(N}_3\text{)}_2 \overset{\Delta}{\rightarrow} \text{Ba} + \text{N}_2 \) is classified as a thermal decomposition redox reaction.

**Final Answer:** The correct classification of the reaction is a thermal decomposition redox reaction.