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Which of the following pairs of ions represent isoelectronic species? A) Mg2* and O² B) K+ and Li+ C) Ca2+ and F- D) Fe2* and S² E) Al3+ and CI

Which of the following pairs of ions represent isoelectronic species? A) Mg2* and O² B) K+ and Li+ C) Ca2+ and F- D) Fe2* and S² E) Al3+ and CI

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Question:** Which of the following pairs of ions represent isoelectronic species? **Options:** A) Mg²⁺ and O²⁻ B) K⁺ and Li⁺ C) Ca²⁺ and F⁻ D) Fe²⁺ and S²⁻ E) Al³⁺ and Cl⁻ **Explanation:** **Isoelectronic species** are atoms, molecules, or ions that have the same number of electrons. This property allows them to exhibit similar electronic configurations and often similar chemical properties with respect to electron-carrying behaviors, even if they are different species. To determine which pairs are isoelectronic, count the electrons in each ion and compare: - **Mg²⁺:** Magnesium originally has 12 electrons. Losing two electrons leaves it with 10 electrons. - **O²⁻:** Oxygen originally has 8 electrons. Gaining two electrons gives it 10 electrons. - **K⁺:** Potassium originally has 19 electrons. Losing one electron leaves it with 18 electrons. - **Li⁺:** Lithium originally has 3 electrons. Losing one electron leaves it with 2 electrons. - **Ca²⁺:** Calcium originally has 20 electrons. Losing two electrons leaves it with 18 electrons. - **F⁻:** Fluorine originally has 9 electrons. Gaining one electron gives it 10 electrons. - **Fe²⁺:** Iron originally has 26 electrons. Losing two electrons leaves it with 24 electrons. - **S²⁻:** Sulfur originally has 16 electrons. Gaining two electrons gives it 18 electrons. - **Al³⁺:** Aluminum originally has 13 electrons. Losing three electrons leaves it with 10 electrons. - **Cl⁻:** Chlorine originally has 17 electrons. Gaining one electron gives it 18 electrons. By matching the electron counts, we see that **option A, Mg²⁺ and O²⁻, are isoelectronic** as they each have 10 electrons.
Transcribed Image Text:**Question:** Which of the following pairs of ions represent isoelectronic species? **Options:** A) Mg²⁺ and O²⁻ B) K⁺ and Li⁺ C) Ca²⁺ and F⁻ D) Fe²⁺ and S²⁻ E) Al³⁺ and Cl⁻ **Explanation:** **Isoelectronic species** are atoms, molecules, or ions that have the same number of electrons. This property allows them to exhibit similar electronic configurations and often similar chemical properties with respect to electron-carrying behaviors, even if they are different species. To determine which pairs are isoelectronic, count the electrons in each ion and compare: - **Mg²⁺:** Magnesium originally has 12 electrons. Losing two electrons leaves it with 10 electrons. - **O²⁻:** Oxygen originally has 8 electrons. Gaining two electrons gives it 10 electrons. - **K⁺:** Potassium originally has 19 electrons. Losing one electron leaves it with 18 electrons. - **Li⁺:** Lithium originally has 3 electrons. Losing one electron leaves it with 2 electrons. - **Ca²⁺:** Calcium originally has 20 electrons. Losing two electrons leaves it with 18 electrons. - **F⁻:** Fluorine originally has 9 electrons. Gaining one electron gives it 10 electrons. - **Fe²⁺:** Iron originally has 26 electrons. Losing two electrons leaves it with 24 electrons. - **S²⁻:** Sulfur originally has 16 electrons. Gaining two electrons gives it 18 electrons. - **Al³⁺:** Aluminum originally has 13 electrons. Losing three electrons leaves it with 10 electrons. - **Cl⁻:** Chlorine originally has 17 electrons. Gaining one electron gives it 18 electrons. By matching the electron counts, we see that **option A, Mg²⁺ and O²⁻, are isoelectronic** as they each have 10 electrons.
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