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Chapter 3: Problem 24

Discuss VSEPR theory and the trend of repulsive interactions in lone pair-lone pair and lone-pairbond pair.

Short Answer

Expert verified
The VSEPR theory predicts the molecular geometry based on the repulsion between electron pairs in the valence shell of an atom. The repulsion follows the trend: lone pair-lone pair > lone pair-bond pair > bond pair - bond pair. This is because lone pairs are located closer to the nucleus and spread out more. This repulsion further affects the shape of the molecule, such as causing a water molecule to have a 'bent' shape.

Step by step solution

01

Understand the VSEPR Theory

The Valence Shell Electron Pair Repulsion (VSEPR) theory is a model in chemistry used to predict the geometry of molecules based on the number of valence electron pairs surrounding their central atoms. Under this theory, electron pairs are treated as charges and will orient themselves so they are as far apart as possible surviving each other's repulsion.
02

Discuss Repulsion Force in Lone Pair-Bond Pair and Lone Pair-Lone Pair

According to VSEPR theory, the pair of electrons in the valence shell experiences repulsive forces from other pairs. This repulsion force follows a hierarchy: Lone pair (LP) - Lone pair repulsion > Lone pair - Bond pair (BP) repulsion > Bond pair - Bond pair repulsion. Lone pairs repel more than bonding pairs because they are closer to the nucleus and spread out more; therefore, they occupy a larger space.
03

Describe the Implication of Repulsion Trend

The trend in repulsion impacts the molecular geometry. For example, a water molecule (H2O) has two bond pairs and two lone pairs around the central oxygen atom. The lone pairs, due to their greater repulsion, push down the bond pairs, resulting in a 'bent' or 'V-shape' molecule despite the four electron pairs theoretically arranging themselves tetrahedrally.

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