Textbook Question
Which neutral atom is isoelectronic with each of the following ions? Ga3+, Zr4+, Mn7+, I−, Pb2+.
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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 Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 7, Problem 30
For each ion, identify the neutral atom that is isoelectronic with it.
a. Cl−
b. Sc3+
c. Fe2+
d. Zn2+
e.Sn4+
Verified step by step guidance1
Identify the number of electrons in each ion.
Determine the number of electrons in the neutral atom by adding or subtracting electrons based on the ion's charge.
For Cl^−, add one electron to the atomic number of Cl to find the isoelectronic neutral atom.
For Sc^3+, subtract three electrons from the atomic number of Sc to find the isoelectronic neutral atom.
Repeat the process for Fe^2+, Zn^2+, and Sn^4+ by adjusting the number of electrons according to their charges to find the isoelectronic neutral atoms.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Isoelectronic Species
Isoelectronic species are atoms or ions that have the same number of electrons, resulting in identical electron configurations. This concept is crucial for identifying which neutral atom corresponds to a given ion, as it allows for the comparison of electron counts rather than atomic numbers.
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03:03
Amphoteric Species
Electron Configuration
Electron configuration describes the distribution of electrons among the various orbitals of an atom or ion. Understanding how to write and interpret electron configurations is essential for determining the number of electrons in an ion and finding the neutral atom that shares the same configuration.
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01:33Electron Configuration Example
Charge of Ions
The charge of an ion indicates the number of electrons lost or gained compared to its neutral atom. For example, a cation like Sc3+ has lost three electrons, while an anion like Cl− has gained one. Recognizing the charge helps in calculating the number of electrons in the ion, which is necessary for identifying the corresponding isoelectronic neutral atom.
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01:39Polyatomic Ion Charges
Related Practice
Textbook Question
Identify each statement as true or false: (b) Li+ is smaller than Li.
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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
For each set of atoms and ions, pick the smallest one.
a. I, I+, I−
b. Be2+, Ca2+, Mg2+
c. Fe, Fe2+, Fe3+
Textbook Question
Consider the isoelectronic ions F- and Na+. (b) Using Equation 7.1 and assuming that core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant, S, calculate Zeff for the 2p electrons in both ions.
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