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 33b,c
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.
Verified step by step guidance1
Step 1: Understand the concept of atomic and ionic sizes. Atomic size refers to the distance between the nucleus of an atom and its outermost shell. Ionic size refers to the size of an atom after it has lost or gained electrons to form an ion.
Step 2: Consider the atomic sizes of S, Cl, and K. In the periodic table, atomic size generally decreases from left to right across a period and increases from top to bottom within a group. Therefore, K (potassium) is larger than S (sulfur) and S is larger than Cl (chlorine).
Step 3: Consider the ionic sizes of S, Cl, and K. The most common ions of these elements are S^2-, Cl-, and K+. When an atom gains electrons to form an anion (like S^2- and Cl-), it becomes larger because the added electrons increase electron-electron repulsion. When an atom loses electrons to form a cation (like K+), it becomes smaller because there are fewer electrons to contribute to electron-electron repulsion.
Step 4: Compare the orders of atomic and ionic sizes. The order of atomic sizes is K > S > Cl. However, the order of ionic sizes is S^2- > Cl- > K+ because S^2- and Cl- gain electrons and become larger, while K+ loses an electron and becomes smaller.
Step 5: Understand the reason for the differences in the orders. The differences in the orders of atomic and ionic sizes are due to the changes in electron-electron repulsion when atoms form ions. Gaining electrons increases electron-electron repulsion and makes an atom larger, while losing electrons decreases electron-electron repulsion and makes an atom smaller.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Atomic Size
Atomic size refers to the distance from the nucleus to the outermost electron shell of an atom. It generally increases down a group in the periodic table due to the addition of electron shells, which outweighs the increase in nuclear charge. Conversely, atomic size decreases across a period as increased nuclear charge pulls electrons closer to the nucleus.
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Atom Structure
Ionic Size
Ionic size is the radius of an ion in a crystal lattice. Cations (positively charged ions) are smaller than their parent atoms because the loss of electrons reduces electron-electron repulsion and allows the remaining electrons to be pulled closer to the nucleus. Anions (negatively charged ions), on the other hand, are larger than their parent atoms due to the addition of electrons, which increases repulsion among electrons.
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Trends in Periodic Table
The periodic table exhibits specific trends in atomic and ionic sizes. As you move from left to right across a period, atomic and ionic sizes generally decrease due to increased nuclear charge. In contrast, moving down a group, both atomic and ionic sizes increase due to the addition of electron shells, which outweighs the effect of increased nuclear charge.
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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
Consider the isoelectronic ions F- and Na+. (c) Repeat this calculation using Slater’s rules to estimate the screening constant, S.
Textbook Question
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.
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