Question:
The molecule with square planar structure containing two lone pairs at the central atom is
The molecule with square planar structure containing two lone pairs at the central atom is
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$XeF_4$ is the classic example of a square planar molecule in main-group chemistry. Its steric number is 6, with 2 lone pairs.
Updated On: Jun 26, 2026
- Platinum(IV) fluoride
- Carbon(IV) fluoride
- Silicon(IV) fluoride
- Xenon (IV) fluoride
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The Correct Option is D
Solution and Explanation
Step 1: Understanding the Concept:
According to VSEPR theory, the molecular shape is determined by the total number of electron pairs (bond pairs + lone pairs) around the central atom.
Step 2: Detailed Explanation:
1. Xenon (IV) fluoride ($XeF_4$):
- Valence electrons of Xe $= 8$.
- Number of bonding fluorine atoms $= 4$.
- Electrons involved in bonding $= 4$.
- Electrons remaining $= 4$ ($2$ lone pairs).
- Total electron pairs $= 4$ (bp) $+ 2$ (lp) $= 6$.
- Hybridization is $sp^3d^2$ (Octahedral geometry).
- With 2 lone pairs, the pairs occupy trans positions to minimize repulsion, resulting in a Square Planar shape.
2. $CF_4$ and $SiF_4$ are tetrahedral ($sp^3$) with no lone pairs.
Step 3: Final Answer:
The molecule is Xenon (IV) fluoride.
According to VSEPR theory, the molecular shape is determined by the total number of electron pairs (bond pairs + lone pairs) around the central atom.
Step 2: Detailed Explanation:
1. Xenon (IV) fluoride ($XeF_4$):
- Valence electrons of Xe $= 8$.
- Number of bonding fluorine atoms $= 4$.
- Electrons involved in bonding $= 4$.
- Electrons remaining $= 4$ ($2$ lone pairs).
- Total electron pairs $= 4$ (bp) $+ 2$ (lp) $= 6$.
- Hybridization is $sp^3d^2$ (Octahedral geometry).
- With 2 lone pairs, the pairs occupy trans positions to minimize repulsion, resulting in a Square Planar shape.
2. $CF_4$ and $SiF_4$ are tetrahedral ($sp^3$) with no lone pairs.
Step 3: Final Answer:
The molecule is Xenon (IV) fluoride.
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