`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 decomposition of lead(II) nitrate (Pb(NO₃)₂) into lead oxide (PbO), nitrogen dioxide (NO₂), and oxygen (O₂), we will follow these steps:

### Step 1: Write the balanced chemical equation
The decomposition reaction can be represented as:
\[ \text{2 Pb(NO}_3\text{)}_2 \xrightarrow{\Delta} \text{2 PbO} + \text{4 NO}_2 + \text{O}_2 \]

### Step 2: Determine the oxidation states of the elements
- In Pb(NO₃)₂:
- Lead (Pb) has an oxidation state of +2.
- Each nitrogen (N) in the nitrate ion (NO₃⁻) has an oxidation state of +5.
- Each oxygen (O) has an oxidation state of -2.

- In the products:
- In PbO, lead (Pb) has an oxidation state of +2 and oxygen (O) is -2.
- In NO₂, nitrogen (N) has an oxidation state of +4.
- In O₂, oxygen (O) has an oxidation state of 0.

### Step 3: Identify changes in oxidation states
- Nitrogen changes from +5 in Pb(NO₃)₂ to +4 in NO₂ (reduction).
- Oxygen changes from -2 in NO₃⁻ to 0 in O₂ (oxidation).

### Step 4: Classify the reaction
- Since there is both oxidation (oxygen) and reduction (nitrogen), this is a redox reaction.
- The reaction is also thermal because it requires heat (Δ) to proceed.
- The reaction involves the breakdown of a single compound (Pb(NO₃)₂) into multiple products, which classifies it as a decomposition reaction.

### Conclusion
The reaction is a **thermal decomposition redox reaction**.