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We can use the vsepr model to predict the geometry of most polyatomic molecules and ions by focusing only on the number of electron pairs around the central atom, ignoring all other valence electrons present. For example a steric number of three gives a trigonal planar electronic shape. In this lesson, you’ll learn how to use vsepr theory to determine molecular shapes—from linear to octahedral—by analyzing electron group repulsions and lone pair effects.

But how do chemists predict the shape of a molecule This number (the steric number) defines the electronic shape of the molecule by minimizing repulsion Enter the valence shell electron pair repulsion (vsepr) theory —a simple, elegant, and surprisingly accurate model that allows us to visualize and predict molecular geometry just by looking at the atoms and their valence electrons.

According to this theory, the molecular shape depends on the repulsion between the valence shell electron pairs of the central atom.

This model assumes that electron pairs will arrange themselves to minimize repulsion effects from one another In other words, the electron pairs are as far apart as possible. According to vsepr theory, the arrangement of valence electrons—both bonded and lone pairs—determines the molecular geometry by causing the electron pairs to position themselves as far apart as possible. Vsepr theory is used to predict the arrangement of electron pairs around central atoms in molecules, especially simple and symmetric molecules.

This article will break down the basics of vsepr theory, key molecular shapes, bond angles, and how electron pair geometry differs from molecular geometry. Vsepr theory helps predict molecular shapes by considering both bonding pairs and lone pairs of electrons, which occupy space around the central atom The most common molecular geometries predicted by vsepr include linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral. We then follow these steps to obtain the electronic geometry

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