**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. The exercise asks you to determine which pair of ions has the same electron count, making them isoelectronic with each other. Consider the atomic numbers and changes in electron count due to ion formation to find the correct pair.

♧ Isoelectronic species : They have same number of electrons as their electronic configuration are same but havedifferent charges . In most of the cases, they have noble gas electronic configuration in order to gain stability . Let's check the given options one by one -A) Mg2+ and O2- :Electronic configuration of Mg : 1s22s22p63s2It loses two electrons from 3s orbital and become Mg2+ ion .Mg2+ : 1s22s22p6Total number of electrons in Mg2+ = 2 + 2 + 6 = 10Electronic configuration of O : 1s22s22p4It gains two electrons in 2p orbital and become O2- ion .O2- : 1s22s22p6Total number of electrons in O2- = 2 + 2 + 6 = 10 Since, they have same number of electrons thus Mg2+ and O2- are isoelectronic species .B) K+ and Li+ :Electronic configuration of K : 1s22s22p63s23p64s1It loses one electron from 4s orbital and becomes K+ ion .K+ : 1s22s22p63s23p6Total number of electrons in K+ = 2 + 2 + 6 + 2 + 6 = 18Electronic configuration of Li : 1s22s1It loses one electron from 2s orbital and becomes Li+ ion .Li+ : 1s2Total number of electrons in Li+ = 2Since, they have different number of electrons thus K+ and Li+ are not isoelectronic species . C) Ca2+ and F- :Electronic configuration of Ca : 1s22s22p63s23p64s2It loses two electrons from 4s orbital and becomes Ca2+ ion .Ca2+ : 1s22s22p63s23p6Total number of electrons in Ca2+ = 2 + 2 + 6 + 2 + 6 = 18Electronic configuration of F: 1s22s22p5It gains one electron in 2p orbital and becomes F- ion .F- : 1s22s22p6Total number of electrons in F- = 2 +2 + 6 = 10Since, they have different number of electrons thus Ca2+ and F- are not isoelectronic species . D) Fe2+ and S2- :Electronic configuration of Fe : 1s22s22p63s23p64s23d6It loses two electrons from 4s orbital and becomes Fe2+ ion .Fe2+ : 1s22s22p63s23p63d6Total number of electrons in Fe2+ = 2 + 2 + 6 + 2 + 6 + 6 = 24Electronic configuration of S : 1s22s22p63s23p4It gains two electrons in 3p orbital and becomes S2- ion .S2- : 1s22s22p63s23p6Total number of electrons in S2- = 2 + 2 + 6 + 2 + 6 = 18Since, they have different number of electrons thus Fe2+ and S2- are not isoelectronic species . E) Al3+ and Cl- :Electronic configuration of Al : 1s22s22p63s23p1It loses three electrons from 3s and 3p orbital and becomes Al3+ ion .Al3+ : 1s22s22p6Total number of electrons in Al3+ = 2 + 2 + 6 = 10Electronic configuration of Cl : 1s22s22p63s23p5It gains one electron in 3p orbital and become Cl- ion .Cl- : 1s22s22p63s23p6Total number of electrons in Cl- = 2 + 2 + 6 + 2 + 6 = 18Since, they have different number of electrons thus Al3+ and Cl- are not isoelectronic species . Hence, Mg2+ and O2- ions represent isoelectronic species .The correct option is - A) Mg2+ and O2-

Answered: Which of the following pairs of ions…

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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 Cl

Chemistry

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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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