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Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Not the one you use?Change textbook
All textbooksTro 5th EditionCh.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO TheoryProblem 52
Chapter 11, Problem 52

Determine whether each molecule is polar or nonpolar. a. SiCl4 b. CF2Cl2 c. SeF6 d. IF5

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Identify the molecular geometry of each molecule using VSEPR theory. This will help in understanding the arrangement of the atoms and the distribution of electron clouds around the central atom.
Determine the electronegativity of each atom in the molecules. Molecules with a significant difference in electronegativity between bonded atoms will have polar bonds.
Analyze the symmetry of the molecule. If the molecule is symmetrical, it is likely nonpolar because the dipole moments cancel out. If it is asymmetrical, the dipole moments do not cancel out, making the molecule polar.
For each molecule, consider the vector sum of the dipole moments. If the vector sum of the dipole moments is zero, the molecule is nonpolar. If the vector sum is not zero, the molecule is polar.
Apply these considerations to each molecule: a. SiCl4, b. CF2Cl2, c. SeF6, d. IF5, to determine if they are polar or nonpolar based on their molecular geometry, electronegativity differences, and symmetry.

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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 significantly influences its polarity, as it determines how bond dipoles (the separation of charge due to differences in electronegativity) are oriented in space. Common geometries include linear, trigonal planar, tetrahedral, and octahedral, each affecting the overall dipole moment of the 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. Understanding the electronegativity values of the atoms involved helps predict the polarity of the bonds and, consequently, the overall polarity of the molecule.
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Dipole Moment

The dipole moment is a vector quantity that represents the separation of positive and negative charges in a molecule. It is calculated as the product of the charge and the distance between the charges. A molecule is considered polar if it has a net dipole moment, meaning that the individual bond dipoles do not cancel out due to the molecule's geometry, resulting in an uneven distribution of electron density.
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Related Practice
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