`Ca(OH)_(2)+Cl_(2) to CaOCl_(2) or Ca(OC l)Cl`

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 reaction \( \text{Ca(OH)}_2 + \text{Cl}_2 \rightarrow \text{Ca(OCl)}_2 \) or \( \text{Ca(OCl)Cl} \), we will analyze the oxidation states of the elements involved in the reaction to determine the type of reaction it is.

### Step-by-step Solution:

1. **Identify the Reactants and Products:**
- Reactants: Calcium hydroxide \( \text{Ca(OH)}_2 \) and chlorine gas \( \text{Cl}_2 \).
- Products: Calcium oxychloride \( \text{Ca(OCl)}_2 \) or \( \text{Ca(OCl)Cl} \).

2. **Assign Oxidation States:**
- In \( \text{Ca(OH)}_2 \):
- Calcium (Ca) = +2
- Oxygen (O) = -2
- Hydrogen (H) = +1
- In \( \text{Cl}_2 \):
- Chlorine (Cl) = 0 (as it is in its elemental form).
- In \( \text{Ca(OCl)}_2 \):
- Calcium (Ca) = +2
- Each oxygen (O) = -2
- Chlorine (Cl) in \( \text{OCl} \) = -1 (since \( \text{Ca} + \text{O} + \text{Cl} = 0 \) leads to \( +2 - 2 + x = 0 \) giving \( x = -1 \)).
- Therefore, in \( \text{Ca(OCl)Cl} \):
- The chlorine outside the bracket is also -1.

3. **Determine Changes in Oxidation States:**
- Chlorine in \( \text{Cl}_2 \) (0) is converted to:
- One chlorine in \( \text{Ca(OCl)}_2 \) is -1 (reduction).
- The other chlorine in \( \text{Ca(OCl)Cl} \) is +1 (oxidation).

4. **Identify the Type of Reaction:**
- Since one species (chlorine) is undergoing both oxidation (from 0 to +1) and reduction (from 0 to -1), this is classified as a **disproportionation reaction**.

5. **Conclusion:**
- The correct classification of the reaction \( \text{Ca(OH)}_2 + \text{Cl}_2 \rightarrow \text{Ca(OCl)}_2 \) or \( \text{Ca(OCl)Cl} \) is a **disproportionation reaction**.

### Final Answer:
The reaction is classified as a **disproportionation reaction**.

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