Question:

Amongst the following which one will have maximum 'lone pair- lone pair' electron repulsions?

Updated On: May 2, 2025

ClF₃
IF₅
SF₄
XeF₂

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The Correct Option is D

Solution and Explanation

The compound with the maximum 'lone pair-lone pair' electron repulsions can be determined by examining the electron configurations and molecular geometry of each molecule. Below is an analysis of each molecule to determine which has the greatest number of lone pairs and thus maximum repulsions:

ClF₃: Chlorine has 7 valence electrons, and forms three bonds with fluorine atoms, leaving behind 2 lone pairs. It has a T-shaped molecular geometry.
IF₅: Iodine has 7 valence electrons and forms five bonds with fluorine atoms, leaving behind 1 lone pair. It has a square pyramidal molecular geometry.
SF₄: Sulfur has 6 valence electrons and forms four bonds with fluorine atoms, leaving behind 1 lone pair. It has a seesaw shape.
XeF₂: Xenon has 8 valence electrons and forms two bonds with fluorine atoms, leaving behind 3 lone pairs. It has a linear geometry.

From this analysis, XeF₂ with 3 lone pairs exhibits the maximum 'lone pair-lone pair' repulsions as each lone pair occupies more space and repels the others strongly. Compared to the other molecules, no other has as many lone pairs, thus XeF₂ will have the maximum repulsions due to its lone pairs.

Conclusion: The molecule XeF₂ has the highest 'lone pair-lone pair' electron repulsions.

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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.