Textbook Question
Identify two ions that have the following ground-state electron configurations: (b) [Ar]3d5
Ch.7 - Periodic Properties of the Elements
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 7, Problem 94c
Identify two ions that have the following ground-state electron configurations: (c) [Kr]5s24d10
Verified step by step guidance1
Identify the given electron configuration: [Kr]5s^2 4d^10.
Recognize that this configuration corresponds to a filled 4d subshell and a filled 5s subshell, which is characteristic of a transition metal ion.
Determine the element with this electron configuration in its neutral state. The configuration [Kr]5s^2 4d^10 corresponds to Cadmium (Cd) in its neutral state.
Consider the possible ions that can be formed by removing electrons from the outermost shell. For Cadmium, the common ion is Cd^2+.
Identify another ion with the same electron configuration. Silver (Ag) can lose one electron to form Ag^+ with the same electron configuration as Cd^2+.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electron Configuration
Electron configuration describes the distribution of electrons in an atom's orbitals. It is represented using a notation that indicates the energy levels and sublevels occupied by electrons. For example, the notation [Kr]5s²4d¹⁰ indicates that the atom has a core configuration similar to krypton, with additional electrons in the 5s and 4d orbitals.
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Electron Configuration Example
Ionic Charge
Ionic charge refers to the electrical charge that an atom or molecule acquires when it loses or gains electrons. Cations are positively charged ions formed by losing electrons, while anions are negatively charged ions formed by gaining electrons. Understanding the ionic charge is essential for identifying ions based on their electron configurations.
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Transition Metals
Transition metals are elements found in the d-block of the periodic table, characterized by their ability to form variable oxidation states and colored compounds. They typically have partially filled d orbitals, which play a crucial role in their chemical behavior. The electron configuration [Kr]5s²4d¹⁰ suggests that the ions in question may be derived from transition metals, which often exhibit complex electron arrangements.
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Related Practice
Textbook Question
Which of the following chemical equations is connected to the definitions of (a) the first ionization energy of oxygen (i) O1g2 + e-¡O-1g2 (ii) O1g2¡O+1g2 + e- (iii) O1g2 + 2 e-¡O2-1g2 (iv) O1g2¡O2+1g2 + 2 e- (v) O+1g2¡O2+1g2 + e-
Textbook Question
The first ionization energy of the oxygen molecule is the energy required for the following process: O21g2¡O2 +1g2 + e- The energy needed for this process is 1175 kJ>mol, very similar to the first ionization energy of Xe. Would you expect O2 to react with F2? If so, suggest a product or products of this reaction.
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Textbook Question
Hydrogen is an unusual element because it behaves in some ways like the alkali metal elements and in other ways like nonmetals. Its properties can be explained in part by its electron configuration and by the values for its ionization energy and electron affinity. (a) Explain why the electron affinity of hydrogen is much closer to the values for the alkali elements than for the halogens.
Textbook Question
Identify two ions that have the following ground-state electron configurations: (a) [Ar]