What is the shape of the cationic part of solid `Cl_2O_6`?

Options

A. Distorted octahedral
B. Square pyramidal
C. Square planar
D. None of these

Answer

To determine the shape of the cationic part of solid Cl₂O₆, we need to analyze its components and hybridization. Here’s a step-by-step solution:

### Step 1: Identify the Cationic and Anionic Parts
The compound Cl₂O₆ can be broken down into its cationic and anionic parts. The cationic part is ClO₂⁺ and the anionic part is ClO₄⁻.

**Hint:** Start by recognizing the components of the compound and separating them into cationic and anionic parts.

### Step 2: Determine the Hybridization of ClO₂⁺
To find the shape of the cation ClO₂⁺, we need to determine its hybridization.

1. Count the total number of valence electrons:
- Chlorine (Cl) has 7 valence electrons.
- Each Oxygen (O) has 6 valence electrons, and there are 2 Oxygens.
- ClO₂⁺ has one less electron due to the positive charge.

Total = 7 + (2 × 6) - 1 = 18 valence electrons.

2. Determine the number of bonding pairs and lone pairs:
- ClO₂⁺ has 2 O atoms bonded to Cl, which accounts for 2 bonding pairs.
- The remaining electrons will be lone pairs on the Cl atom.

Since 2 bonding pairs use 4 electrons, we have 14 electrons left. These will be distributed as lone pairs.

3. The central Cl atom will have 2 bonding pairs and 1 lone pair (since 2 bonding pairs use 4 electrons and we have 18 total).

**Hint:** Calculate the total valence electrons and determine how they are distributed between bonding and lone pairs.

### Step 3: Determine the Shape Using VSEPR Theory
According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the arrangement of electron pairs around the central atom determines the molecular geometry.

- With 2 bonding pairs and 1 lone pair, the geometry is based on the arrangement of 3 regions of electron density.
- The shape is classified as "bent" or "angular" due to the presence of the lone pair which pushes the bonding pairs closer together.

**Hint:** Use VSEPR theory to relate the number of bonding pairs and lone pairs to the molecular shape.

### Step 4: Conclusion
The shape of the cationic part ClO₂⁺ is bent or angular due to the presence of one lone pair and two bonding pairs.

**Final Answer:** The shape of the cationic part of solid Cl₂O₆ (ClO₂⁺) is bent.