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Identify the elements correctly shown by decreasing radii size. Cu²+ > Cut OK+ > K ON ³-> N ON>№ ³- OS > S²-

Identify the elements correctly shown by decreasing radii size. Cu²+ > Cut OK+ > K ON ³-> N ON>№ ³- OS > S²-

Living by Chemistry
Living by Chemistry
2nd Edition
ISBN:9781464142314
Author:Angelica M. Stacy
Publisher:Angelica M. Stacy
ChapterU2: Smells: Molecular Structure And Properties
Section: Chapter Questions
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### Understanding Ionic Radii Atoms and ions differ in size, primarily depending on their electrical charge. When an atom loses or gains electrons, it forms ions that are either smaller or larger than the original atom due to the change in the number of electrons and the resulting electron-electron repulsion forces. The prompt in the image asks to "Identify the elements correctly shown by decreasing radii size." Below are the options provided: 1. ⃝ Cu²⁺ > Cu⁺ 2. ⃝ K⁺ > K 3. ⃝ N³⁻ > N 4. ⃝ N > N³⁻ 5. ⃝ S⁻ > S²⁻ ### Explanation: 1. **Cu²⁺ > Cu⁺**: This option suggests that a copper ion with a 2+ charge is larger than a copper ion with a 1+ charge. However, losing more electrons (i.e., going from Cu⁺ to Cu²⁺) typically results in a smaller ionic radius due to less electron-electron repulsion and increased effective nuclear charge. Hence, this option is incorrect. 2. **K⁺ > K**: This option posits that a potassium ion with a 1+ charge is larger than a neutral potassium atom. However, K⁺ has lost an electron, leading to a smaller ionic radius compared to the neutral K atom. Hence, this option is incorrect. 3. **N³⁻ > N**: This suggests that a nitrogen ion with a 3- charge is larger than a neutral nitrogen atom. This is true, as adding electrons (going from N to N³⁻) increases electron-electron repulsion, resulting in a larger ionic radius. Hence, this option is correct. 4. **N > N³⁻**: This suggests that a neutral nitrogen atom is larger than a nitrogen ion with a 3- charge. However, gaining electrons increases the ionic radius due to electron-electron repulsion, meaning a neutral N atom would be smaller than N³⁻. Hence, this option is incorrect. 5. **S⁻ > S²⁻**: This option suggests a sulfur ion with a 1- charge is larger than a sulfur ion with a 2- charge. However, adding more electrons (going from S⁻ to S²⁻) increases electron-electron repulsion
Transcribed Image Text:### Understanding Ionic Radii Atoms and ions differ in size, primarily depending on their electrical charge. When an atom loses or gains electrons, it forms ions that are either smaller or larger than the original atom due to the change in the number of electrons and the resulting electron-electron repulsion forces. The prompt in the image asks to "Identify the elements correctly shown by decreasing radii size." Below are the options provided: 1. ⃝ Cu²⁺ > Cu⁺ 2. ⃝ K⁺ > K 3. ⃝ N³⁻ > N 4. ⃝ N > N³⁻ 5. ⃝ S⁻ > S²⁻ ### Explanation: 1. **Cu²⁺ > Cu⁺**: This option suggests that a copper ion with a 2+ charge is larger than a copper ion with a 1+ charge. However, losing more electrons (i.e., going from Cu⁺ to Cu²⁺) typically results in a smaller ionic radius due to less electron-electron repulsion and increased effective nuclear charge. Hence, this option is incorrect. 2. **K⁺ > K**: This option posits that a potassium ion with a 1+ charge is larger than a neutral potassium atom. However, K⁺ has lost an electron, leading to a smaller ionic radius compared to the neutral K atom. Hence, this option is incorrect. 3. **N³⁻ > N**: This suggests that a nitrogen ion with a 3- charge is larger than a neutral nitrogen atom. This is true, as adding electrons (going from N to N³⁻) increases electron-electron repulsion, resulting in a larger ionic radius. Hence, this option is correct. 4. **N > N³⁻**: This suggests that a neutral nitrogen atom is larger than a nitrogen ion with a 3- charge. However, gaining electrons increases the ionic radius due to electron-electron repulsion, meaning a neutral N atom would be smaller than N³⁻. Hence, this option is incorrect. 5. **S⁻ > S²⁻**: This option suggests a sulfur ion with a 1- charge is larger than a sulfur ion with a 2- charge. However, adding more electrons (going from S⁻ to S²⁻) increases electron-electron repulsion
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