Question:

The shape of XeOF4 molecule is:

Updated On: Apr 7, 2025

  •  Square pyramid

  •  Planar

  •  Trigonal bipyramid

  •  Pentagonal bipyramid 

  •  Linear 

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The Correct Option is A

Approach Solution - 1

XeOF4 VSEPR analysis:

  • Central Xe with 5 bond pairs (4 F + 1 O) and 1 lone pair
  • AX5E configuration (octahedral electron geometry)
  • Lone pair occupies axial position → Square pyramidal molecular shape

Thus, the correct option is (A): Square pyramid.

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Approach Solution -2

1. Analyze the structure of \( \text{XeOF}_4 \):

To determine the shape of the \( \text{XeOF}_4 \) molecule, we use the **VSEPR (Valence Shell Electron Pair Repulsion) theory**. The steps are as follows:

  • Xenon (\( \text{Xe} \)) is the central atom in \( \text{XeOF}_4 \).
  • Xenon has 8 valence electrons.
  • In \( \text{XeOF}_4 \), xenon forms:
    • One double bond with oxygen (\( \text{O} \)), which counts as one electron pair.
    • Four single bonds with four fluorine (\( \text{F} \)) atoms, which count as four electron pairs.
  • The remaining two electrons on xenon exist as a lone pair.
  • Thus, there are a total of **6 electron pairs** around the central xenon atom: 5 bonding pairs and 1 lone pair.

2. Determine the hybridization and geometry:

  • With 6 electron pairs around the central atom, the hybridization is \( \text{sp}^3\text{d}^2 \).
  • The electron geometry is **octahedral**, as six electron pairs arrange themselves to minimize repulsion.
  • However, the molecular shape depends only on the positions of atoms, not lone pairs. With one lone pair, the shape becomes a **square pyramid**.

3. Match the result with the given options:

  • The shape of \( \text{XeOF}_4 \) is square pyramid, which corresponds to Option (A).

4. Final answer:

The correct option is (A) Square pyramid.

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Concepts Used:

VSEPR theory

The Valence Shell Electron Pair Repulsion Theory abbreviated as VSEPR theory is based on the premise that there is a repulsion between the pairs of valence electrons in all atoms, and the atoms will always tend to arrange themselves in a manner in which this electron pair repulsion is minimalized.

Postulates of Valence Bond Theory

  • The overlapping of two half-filled valence orbitals of two different atoms forms the covalent bond. The electron density between two linked atoms increases due to the overlapping. The molecule thus gains the property of stability.
  • More than one bond can be created if the atomic orbitals contain more than one unpaired electron. As per the valence bond theory, the paired electrons in the valence shell cannot participate in such bond formation.
  • A covalent bond has a specific direction. The region of overlapping atomic orbitals is also parallel to such a bond.
  • There are two types of covalent bonds based on the overlapping pattern: sigma bonds and pi bonds. The pi bond is formed by the overlapping of atomic orbitals sideways, whereas the sigma bond is created by the overlapping of atomic orbitals along the axis of the nucleus.

Types of Hybrid Orbitals:

Applications of Valence Bond Theory

  • The maximum overlap conditions which is given by the valence bond theory can explain the formation of covalent bonds in many compounds.
  • One of its most important applications is the variation in the length and strength of chemical bonds in H2 and F2 molecules can be explained by the difference in their overlapping orbitals.
  • The overlap of the 1s orbital of the hydrogen atom and the 2p orbital of the fluorine atom makes the covalent bond in an HF molecule which is explained by the valence bond theory.

Limitations of the VSEPR theory

  • The VSEPR model is not a theory. It does not explain or attempt to explain any observations or predictions. Rather, it is an algorithm that accurately predicts the structures of a large number of compounds.
  • VSEPR is simple and useful but does not work for all chemical species.
  • First, the idealized bond angles do not always match the measured values. For example, VSEPR predicts that and will have the same bond angles, but structural studies have shown the bonds in the two molecules are different by 12 degrees.
  • VSEPR also predicts that group-2 halides such as will be linear when they are actually bent. Quantum mechanics and atomic orbitals can give more sophisticated predictions when VSEPR is inadequate.