The compound in which the number of `d pi - p pi` bonds are equal to those present in `ClO_(4)^(-)`

Options

A. `XeF_4`
B. `XeO_3`
C. `XeO_4`
D. `XeF_6`

Answer

To solve the problem of finding the compound in which the number of dπ - pπ bonds are equal to those present in ClO₄⁻, we will follow these steps:

### Step 1: Analyze ClO₄⁻
- ClO₄⁻ (chlorate ion) has a central chlorine atom bonded to four oxygen atoms.
- The structure can be represented as one chlorine atom double bonded to three oxygen atoms and single bonded to one oxygen atom that carries a negative charge.
- This results in a total of **three dπ - pπ bonds** (the double bonds).

### Step 2: Identify the Hybridization of ClO₄⁻
- The hybridization of ClO₄⁻ is **sp³** since it has four bond pairs and no lone pairs on the chlorine atom.

### Step 3: Identify Compounds with Similar dπ - pπ Bonds
- We need to find a compound that also has **three dπ - pπ bonds**.
- Let's analyze the given options one by one.

### Step 4: Analyze the Options
1. **Option 1: XeF₄**
- XeF₄ has a square planar geometry with four Xe-F single bonds and no dπ - pπ bonds. **(0 dπ - pπ bonds)**

2. **Option 2: XeO₃**
- XeO₃ has three double bonds with oxygen and one lone pair on xenon. This results in **three dπ - pπ bonds**. **(3 dπ - pπ bonds)**

3. **Option 3: XeO₄**
- XeO₄ has four double bonds with oxygen and no lone pairs on xenon. This results in **four dπ - pπ bonds**. **(4 dπ - pπ bonds)**

### Step 5: Conclusion
- The only compound with the same number of dπ - pπ bonds as ClO₄⁻ (which has three) is **XeO₃**.
- Therefore, the answer is **Option 2: XeO₃**.

### Summary of Steps:
1. Analyze ClO₄⁻ and determine the number of dπ - pπ bonds.
2. Identify the hybridization of ClO₄⁻.
3. Analyze the provided options for their bonding characteristics.
4. Conclude which compound has the same number of dπ - pπ bonds as ClO₄⁻.