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Which of the followings is an isoelectronic series?

Which of the followings is an isoelectronic series?

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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### Isoelectronic Series Identification **Question:** Which of the followings is an isoelectronic series? **Options:** - O C, Si, Ge, Sn - O O²⁻, Li⁺, Be²⁺, Ne - O Al³⁺, Ga³⁺, In³⁺, Tl³⁺ - O Xe, Te²⁻, Cs⁺, I⁻ - O P, S, Cl, Ar **Explanation:** An isoelectronic series refers to a group of atoms, ions, or molecules that have the same number of electrons. This occurs when the entities involved share the same electron configuration despite potentially having different nuclear charges. **Detailed Analysis of Options:** 1. **C, Si, Ge, Sn**: - These are elements from the same group in the periodic table, but they do not have the same number of electrons in their neutral and ionized forms. 2. **O²⁻, Li⁺, Be²⁺, Ne**: - O²⁻ has 10 electrons (8 protons + 2 extra electrons) - Li⁺, with 1 less electron, also has 2 electrons (3 protons minus 1 electron), - Be²⁺ has 2 fewer electrons, making 2 electrons (4 protons minus 2 electrons), - Ne is a noble gas with 10 electrons. - So, they do not form an isoelectronic series because they have different numbers of electrons. 3. **Al³⁺, Ga³⁺, In³⁺, Tl³⁺**: - These ions typically share the same valence configuration because they lose the same number of electrons to achieve a stable structure. 4. **Xe, Te²⁻, Cs⁺, I⁻**: - All these ions and the neutral atom share the configuration of xenon (Xe), implying they have an identical number of electrons when ionized appropriately. 5. **P, S, Cl, Ar**: - These are sequential elements within the same period possessing different electrons in neutral states. **Correct Answer:** - **Xe, Te²⁻, Cs⁺, I⁻** This set forms an isoelectronic series as all listed ions and the atom share the
Transcribed Image Text:### Isoelectronic Series Identification **Question:** Which of the followings is an isoelectronic series? **Options:** - O C, Si, Ge, Sn - O O²⁻, Li⁺, Be²⁺, Ne - O Al³⁺, Ga³⁺, In³⁺, Tl³⁺ - O Xe, Te²⁻, Cs⁺, I⁻ - O P, S, Cl, Ar **Explanation:** An isoelectronic series refers to a group of atoms, ions, or molecules that have the same number of electrons. This occurs when the entities involved share the same electron configuration despite potentially having different nuclear charges. **Detailed Analysis of Options:** 1. **C, Si, Ge, Sn**: - These are elements from the same group in the periodic table, but they do not have the same number of electrons in their neutral and ionized forms. 2. **O²⁻, Li⁺, Be²⁺, Ne**: - O²⁻ has 10 electrons (8 protons + 2 extra electrons) - Li⁺, with 1 less electron, also has 2 electrons (3 protons minus 1 electron), - Be²⁺ has 2 fewer electrons, making 2 electrons (4 protons minus 2 electrons), - Ne is a noble gas with 10 electrons. - So, they do not form an isoelectronic series because they have different numbers of electrons. 3. **Al³⁺, Ga³⁺, In³⁺, Tl³⁺**: - These ions typically share the same valence configuration because they lose the same number of electrons to achieve a stable structure. 4. **Xe, Te²⁻, Cs⁺, I⁻**: - All these ions and the neutral atom share the configuration of xenon (Xe), implying they have an identical number of electrons when ionized appropriately. 5. **P, S, Cl, Ar**: - These are sequential elements within the same period possessing different electrons in neutral states. **Correct Answer:** - **Xe, Te²⁻, Cs⁺, I⁻** This set forms an isoelectronic series as all listed ions and the atom share the
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