Textbook Question
Draw sketches illustrating the overlap between the following orbitals on two atoms: (a) the 2s orbital on each atom
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Ch.9 - Molecular Geometry and Bonding Theories
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 9, Problem 41
Predict whether each of the following molecules is polar or nonpolar: (a) IF, (b) CS2, (c) SO3, (d) PCl3, (e) SF6, (f) IF5.
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Determine the molecular geometry for each molecule using VSEPR theory.
Assess the electronegativity difference between the atoms in each molecule to identify polar bonds.
For each molecule, evaluate the symmetry of the molecular geometry to determine if the dipoles cancel out.
If the dipoles do not cancel out, the molecule is polar; if they do, the molecule is nonpolar.
Summarize the polarity of each molecule based on the analysis of bond polarity and molecular geometry.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Polarity
Molecular polarity refers to the distribution of electrical charge across a molecule, which determines whether it has a positive or negative end. A molecule is polar if it has a significant difference in electronegativity between its atoms, leading to an uneven distribution of charge. Nonpolar molecules, on the other hand, have an even distribution of charge, often due to symmetrical arrangements of identical atoms or balanced dipoles.
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Molecular Polarity
Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. The difference in electronegativity between two bonded atoms can indicate whether the bond is ionic, polar covalent, or nonpolar covalent. In general, larger differences in electronegativity (greater than 1.7) result in ionic bonds, while smaller differences (less than 1.7) can lead to polar or nonpolar covalent bonds.
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Molecular Geometry
Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. The shape of a molecule affects its polarity; for example, a symmetrical shape can lead to nonpolar characteristics even if the individual bonds are polar. Understanding the geometry, often predicted by VSEPR theory, is crucial for determining the overall polarity of a molecule, as it influences how dipoles from polar bonds interact.
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Related Practice
Textbook Question
(b) It turns out that ozone, O3, has a small dipole moment. How is this possible, given that all the atoms are the same?
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Textbook Question
a. Consider the AF3 molecules in Exercise 9.27. Which of these will have a nonzero dipole moment?
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Textbook Question
Dichloroethylene (C2H2Cl2) has three forms (isomers), each of which is a different substance. (b) Which of these isomers has a zero dipole moment?
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Textbook Question
(c) Does the molecule BF2Cl have a dipole moment?
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Textbook Question
Predict whether each of the following molecules is polar or nonpolar: (a) CCl4, (b) NH3, (c) SF4, (d) XeF4, (e) CH3Br, (f) GaH3.
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