The decomposition of `KClO_(3)` to KCl and `O_(2)` on heating is an example of :

Options

A. Intermolecular redox change
B. Intramolecular redox change
C. Disproportionation or auto redox change
D. None

Answer

To determine the type of change that occurs during the decomposition of potassium chlorate (KClO₃) into potassium chloride (KCl) and oxygen (O₂) upon heating, we can analyze the oxidation states of the elements involved in the reaction.

### Step-by-Step Solution:

1. **Write the decomposition reaction:**
The decomposition of potassium chlorate can be represented as:
\[ 2 \text{KClO}_3 \rightarrow 2 \text{KCl} + 3 \text{O}_2 \]

2. **Assign oxidation states:**
- In KClO₃:
- Potassium (K) has an oxidation state of +1.
- Chlorine (Cl) has an oxidation state of +5.
- Oxygen (O) has an oxidation state of -2.
- In KCl:
- Potassium (K) has an oxidation state of +1.
- Chlorine (Cl) has an oxidation state of -1.
- In O₂:
- Oxygen (O) has an oxidation state of 0.

3. **Identify changes in oxidation states:**
- **For Chlorine (Cl):**
- Changes from +5 in KClO₃ to -1 in KCl.
- This is a reduction (gain of electrons).
- **For Oxygen (O):**
- Changes from -2 in KClO₃ to 0 in O₂.
- This is an oxidation (loss of electrons).

4. **Determine the type of redox change:**
Since one element (chlorine) is reduced while another element (oxygen) is oxidized within the same compound (KClO₃), this process is classified as an **intramolecular redox change**.

5. **Conclusion:**
The correct answer is:
- **Option B: Intramolecular redox change.**