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Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory
Chapter 11, Problem 52

Determine whether each molecule is polar or nonpolar.
a. IF5
b. SCl2
c. SCl4
d. BrF5

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. The shape of a molecule is determined by the number of bonding pairs and lone pairs of electrons around the central atom, which can be predicted using the VSEPR (Valence Shell Electron Pair Repulsion) theory. Understanding the geometry is crucial for determining the polarity of a molecule.
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Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. Differences in electronegativity between bonded atoms can lead to polar covalent bonds, where electrons are shared unequally. This concept is essential for assessing whether a molecule has a dipole moment, which contributes to its overall polarity.
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Dipole Moment

A dipole moment is a vector quantity that represents the separation of positive and negative charges in a molecule. It occurs when there is an uneven distribution of electron density, often due to differences in electronegativity. A molecule is considered polar if it has a net dipole moment, while nonpolar molecules have symmetrical charge distributions that cancel out any dipole moments.
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