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Chapter 6: Problem 26

Why do electron pairs around a central atom stay as far apart as possible?

Short Answer

Expert verified
Electron pairs around a central atom stay as far apart as possible due to the phenomenon known as electron-pair repulsion, explained by VSEPR theory. This happens because electrons carry the same charge, and same charges repel each other. This repulsion determines the shape of the molecules as the formation that minimizes the repulsion between electron pairs is the most stable.

Step by step solution

01

Understand the structure of a molecule

Atoms form molecules in order to be more stable. They do this by sharing electrons, and each atom wants to have its electron cloud filled as much as possible. This could be visualized with a central atom surrounded by electron pairs. Each electron pair would like to be as far from other electron pairs as possible, creating a certain 3D structure.
02

Define Electron Pair Repulsion

This phenomenon is explained by the Valence Shell Electron Pair Repulsion (VSEPR) theory, which states that electron pairs arrange themselves around the central atom in a way that they stay as far apart as possible. Why? This is due to fact electrons have same charges and by physics law, same charges repel each other. As a result, structures of molecules are determined by this repulsion that keeps pairs of electrons as far apart as possible.
03

Explain the effect on the molecular structure

By trying to decrease the repulsion between electron pairs the central atom spreads them as wide as possible. This effect significantly influences the shape of molecules, as the angle between bonds is determined by how these electron pairs minimize their repulsion. Ultimately, this leads to the most stable formation, or geometrical structure, of the molecule.

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