`Pb(NO_(3))_(2) overset(Delta)to PbO+NO_(2)+O_(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 solve the question regarding the thermal decomposition of lead(II) nitrate (Pb(NO₃)₂) into lead(II) oxide (PbO), nitrogen dioxide (NO₂), and oxygen (O₂), we will analyze the reaction step by step.

### Step-by-Step Solution:

1. **Identify the Reaction Type**:
- The reaction involves heating lead(II) nitrate, which results in the formation of multiple products from a single reactant.
- This indicates that the reaction is a **thermal decomposition reaction**.

2. **Write the Balanced Chemical Equation**:
- The unbalanced equation is:
\[ \text{Pb(NO}_3\text{)}_2 \xrightarrow{\Delta} \text{PbO} + \text{NO}_2 + \text{O}_2 \]
- To balance the equation, we need to ensure that the number of each type of atom is the same on both sides. The balanced equation is:
\[ 2 \text{Pb(NO}_3\text{)}_2 \xrightarrow{\Delta} 2 \text{PbO} + 4 \text{NO}_2 + \text{O}_2 \]

3. **Determine Oxidation States**:
- Assign oxidation states to each element in the reactants and products:
- In Pb(NO₃)₂:
- Pb = +2
- N in NO₃ = +5
- O in NO₃ = -2
- In PbO:
- Pb = +2
- O = -2
- In NO₂:
- N = +4
- O = -2
- In O₂:
- O = 0 (elemental form)

4. **Analyze Changes in Oxidation States**:
- Lead (Pb) remains at +2 in both reactants and products (no change).
- Nitrogen (N) changes from +5 in Pb(NO₃)₂ to +4 in NO₂ (reduction).
- Oxygen (O) changes from -2 in NO₃ to 0 in O₂ (oxidation).

5. **Determine if the Reaction is a Redox Reaction**:
- Since nitrogen is reduced (decrease in oxidation state) and oxygen is oxidized (increase in oxidation state), this indicates that the reaction is indeed a **redox reaction**.

6. **Conclusion**:
- The reaction is a **thermal decomposition reaction** and also a **redox reaction**. Therefore, the correct answer to the question is option 4.