Textbook Question
Arrange the bonds in each of the following sets in order of increasing polarity: (c) C—S, B—F, N—O.
Ch.8 - Basic Concepts of Chemical Bonding
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 8, Problem 42a,b
Arrange the bonds in each of the following sets in order of increasing polarity: (a) C—F, O—F, Be—F (b) O—Cl,S—Br, C—P
Verified step by step guidance1
Identify the electronegativity values for each element involved in the bonds: O, Cl, S, Br, C, and P.
Calculate the electronegativity difference for each bond: O—Cl, S—Br, and C—P.
Recall that the greater the difference in electronegativity between two atoms, the more polar the bond.
Compare the calculated electronegativity differences to determine the order of increasing polarity.
Arrange the bonds from the smallest to the largest electronegativity difference, indicating increasing polarity.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. The greater the difference in electronegativity between two bonded atoms, the more polar the bond will be. For example, oxygen is more electronegative than chlorine, leading to a polar bond in O—Cl.
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Bond Polarity
Bond polarity refers to the distribution of electrical charge across a bond between two atoms. A bond is considered polar if there is a significant difference in electronegativity between the two atoms, resulting in a dipole moment. Nonpolar bonds occur when atoms have similar electronegativities, leading to an even distribution of charge.
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Comparative Bond Analysis
Comparative bond analysis involves evaluating the bonds based on their electronegativity differences to determine their relative polarities. By comparing the electronegativities of the atoms involved in each bond, one can rank the bonds from least to most polar. This analysis is essential for understanding the behavior of molecules in various chemical contexts.
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Related Practice
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(b) If you were to put HBr under very high pressure, so its bond length decreased significantly, would its dipole moment increase, decrease, or stay the same, if you assume that the effective charges on the atoms do not change?
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(a) From the data in Table 8.2, calculate the effective charges on the H atom of the HBr molecule in units of the electronic charge, e.
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By referring only to the periodic table, select (d) the element in the group K, C, Zn, F that is most likely to form an ionic compound with Ba.
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By referring only to the periodic table, select (a) the most electronegative element in group 13; (b) the least electronegative element in the group As, Se and Br;
Textbook Question
Which of the following bonds are polar? (a) C—O, (b) Sl—F, (c) N—Cl, (d) C—Cl. Which is the more electronegative atom in each polar bond?