Textbook Question
Why is energy usually released when an electron is added to a neutral atom but absorbed when an electron is removed from a neutral atom?
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Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
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McMurry 8th EditionCh.6 - Ionic Compounds: Periodic Trends and Bonding TheoryProblem 67
McMurry 8th EditionCh.6 - Ionic Compounds: Periodic Trends and Bonding TheoryProblem 67Chapter 6, Problem 67
What is the relationship between the ionization energy of a singly charged anion such as Cl- and the electron affinity of the neutral atom?
Verified step by step guidance1
Understand that ionization energy is the energy required to remove an electron from an atom or ion, while electron affinity is the energy change when an electron is added to a neutral atom.
Recognize that for a singly charged anion like Cl-, ionization energy refers to the energy needed to remove the extra electron, converting it back to a neutral atom.
Note that the electron affinity of a neutral atom, such as Cl, is the energy released when an electron is added to form the anion Cl-.
Realize that the ionization energy of Cl- is numerically equal to the negative of the electron affinity of Cl, because the processes are essentially the reverse of each other.
Conclude that the relationship between the ionization energy of Cl- and the electron affinity of Cl is that they are equal in magnitude but opposite in sign.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ionization Energy
Ionization energy is the energy required to remove an electron from a gaseous atom or ion. For anions, such as Cl<sup>-</sup>, the ionization energy reflects the stability of the extra electron. A higher ionization energy indicates that the electron is held more tightly, making it more difficult to remove.
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Ionization Energy
Electron Affinity
Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gas phase. It quantifies how much energy is released or absorbed when an atom gains an electron. A more negative electron affinity means that the atom more readily accepts an electron, contributing to the formation of anions.
Relationship Between Ionization Energy and Electron Affinity
The relationship between ionization energy and electron affinity is crucial in understanding anion stability. For a singly charged anion like Cl<sup>-</sup>, the ionization energy is typically lower than the electron affinity of the neutral atom. This indicates that while the atom can easily gain an electron (high electron affinity), removing that electron from the anion requires a significant amount of energy.