Question

The molecule with square planar structure containing two lone pairs at the central atom is

• A. Platinum(IV) fluoride
• B. Carbon(IV) fluoride
• C. Silicon(IV) fluoride
• D. Xenon (IV) fluoride

Hint:

$XeF_4$ is the classic example of a square planar molecule in main-group chemistry. Its steric number is 6, with 2 lone pairs.

Answer 1

The Correct Option is D

Step 1: Understanding the Concept:
According to VSEPR theory, the geometry of a molecule is determined by the total number of bond pairs and lone pairs around the central atom.
Step 2: Key Formula or Approach:
For Xenon (IV) fluoride (XeF\textsubscript{4}):
- Valence electrons of Xe = 8.
- Number of bonding atoms (F) = 4.
- Total electron pairs = \( \frac{8 + 4}{2} = 6 \).
- Lone pairs = \( 6 - 4 = 2 \).
Step 3: Detailed Explanation:
1. The hybridization is sp{3}d{2} because there are 6 electron pairs.
2. The electron geometry is octahedral.
3. To minimize repulsion (Lone Pair-Lone Pair), the two lone pairs are placed at axial positions (opposite to each other).
4. The remaining 4 bonding atoms (Fluorines) occupy the equatorial positions, resulting in a square planar molecular geometry.
5. Other options like CF\textsubscript{4} and SiF\textsubscript{4} are tetrahedral (4 bp, 0 lp).
Step 4: Final Answer:
The molecule is Xenon (IV) fluoride (XeF\textsubscript{4}).