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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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 37a
a. Does SCl2 have a nonzero dipole moment?
Verified step by step guidance1
Identify the molecular geometry of SCl_2. Sulfur dichloride (SCl_2) has a bent shape due to the presence of lone pairs on the sulfur atom.
Determine the electronegativity of the atoms involved. Chlorine is more electronegative than sulfur, which means the S-Cl bonds are polar.
Consider the vector sum of the dipole moments. In a bent molecular geometry, the dipole moments do not cancel out completely.
Assess the symmetry of the molecule. Since SCl_2 is not symmetrical, the dipole moments do not cancel each other out.
Conclude that SCl_2 has a nonzero dipole moment due to its bent shape and polar bonds.
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 influences the overall polarity. For SCl2, the bent shape due to the presence of lone pairs on sulfur is crucial for understanding its dipole moment.
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01:33
Molecular Geometry with Two Electron Groups
Polarity and Dipole Moment
Polarity in molecules arises from differences in electronegativity between bonded atoms, leading to uneven distribution of electron density. A dipole moment is a vector quantity that measures the separation of positive and negative charges in a molecule. If a molecule has an asymmetrical shape and polar bonds, it will have a nonzero dipole moment, indicating that it is polar.
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01:25Dipole Moment
Electronegativity
Electronegativity is the tendency of an atom to attract electrons in a chemical bond. In SCl2, sulfur has a lower electronegativity than chlorine, resulting in polar S-Cl bonds. The difference in electronegativity contributes to the overall dipole moment of the molecule, as the unequal sharing of electrons leads to a partial positive charge on sulfur and a partial negative charge on chlorine.
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02:10Electronegativity Trends
Related Practice
Textbook Question
Consider the following XF4 ions: PF4-, BrF4-, ClF4+, and AlF4-. (c) Which of the ions will have an octahedral electron-domain geometry?
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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
(c) Does the molecule BF2Cl have a dipole moment?
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