Textbook Question
(a) What is the general relationship between the size of an atom and its first ionization energy?
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Ch.7 - Periodic Properties of the Elements
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 7, Problem 36b
In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation–anion distances are 201 pm (Li–F), 282 pm (Na–Cl), 330 pm (K–Br), and 367 pm (Rb–I), respectively. (b) Calculate the difference between the experimentally measured ion–ion distances and the ones predicted from Figure 7.8.
Verified step by step guidance1
Identify the ionic radii of the cations and anions from the provided table: Li+ (90 pm), Na+ (116 pm), K+ (152 pm), Rb+ (166 pm), F- (119 pm), Cl- (167 pm), Br- (182 pm), I- (206 pm).
Calculate the predicted ion–ion distances by adding the radii of the respective cations and anions: LiF (Li+ + F-), NaCl (Na+ + Cl-), KBr (K+ + Br-), RbI (Rb+ + I-).
Compare the experimentally measured ion–ion distances with the predicted distances: LiF (201 pm), NaCl (282 pm), KBr (330 pm), RbI (367 pm).
Determine the difference between the experimentally measured distances and the predicted distances for each compound.
Summarize the differences for each compound: LiF, NaCl, KBr, and RbI.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ionic Radii
Ionic radii refer to the effective size of an ion in a crystal lattice, which is influenced by its charge and the number of electrons. Cations, which are positively charged, are generally smaller than their neutral atoms due to the loss of electrons, while anions, negatively charged, are larger due to the addition of electrons. Understanding ionic radii is crucial for predicting the distances between ions in ionic compounds.
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Cation-Anion Distances
Cation-anion distances are the measured distances between the centers of cations and anions in an ionic compound. These distances can be experimentally determined and are influenced by the sizes of the ions involved. Analyzing these distances helps in understanding the stability and structure of ionic compounds, as well as their physical properties.
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Experimental vs. Predicted Values
In chemistry, comparing experimental values with predicted values allows for the validation of theoretical models. In this context, the predicted ion-ion distances can be derived from the ionic radii, while the experimental values are obtained through measurement. Discrepancies between these values can provide insights into the nature of ionic bonding and the arrangement of ions in the crystal lattice.
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Related Practice
Textbook Question
Identify each statement as true or false:(a) Ionization energies are always endothermic.(b) Potassium has a larger first ionization energy than lithium.(c) The second ionization energy of the sodium atom is larger than the second ionization energy of the magnesium atom.(d) The third ionization energy is three times the first ionization energy of an atom.
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Textbook Question
Consider S, Cl, and K and their most common ions. (a) List the atoms in order of increasing size.
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Textbook Question
(b) Which element in the periodic table has the largest ionization energy? Which has the smallest?
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Textbook Question
Consider S, Cl, and K and their most common ions. (b) List the ions in order of increasing size. (c) Explain any differences in the orders of the atomic and ionic sizes.
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