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Aufbau violation 2p 111 2p 111 2s1 2s 3p 1.1 3s 1 Hund violation 4d1111 5s 1 5s 3d 1 1 1 1 1 4s Pauli violation

Aufbau violation 2p 111 2p 111 2s1 2s 3p 1.1 3s 1 Hund violation 4d1111 5s 1 5s 3d 1 1 1 1 1 4s Pauli violation

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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Classify each orbital diagram for ground-state electron configurations by the rule or principle it violates.
The image displays diagrams illustrating electron configurations and potential violations of electron filling principles. ### Electron Configurations: 1. **First Diagram:** - **2s Orbital:** Two electrons with opposing spins. - **2p Orbital:** Three electrons with parallel spins in separate boxes. 2. **Second Diagram:** - **2s Orbital:** One electron. - **2p Orbital:** Three electrons with parallel spins in separate boxes. 3. **Third Diagram:** - **3s Orbital:** Two electrons with opposing spins. - **3p Orbital:** Three electrons, one pair with opposing spins and one single electron. 4. **Fourth Diagram:** - **4d Orbital:** Five electrons, three pairs and one single electron, with opposing spins depicted. - **5s Orbital:** Two electrons with opposing spins. 5. **Fifth Diagram:** - **4s Orbital:** Two electrons with opposing spins. - **3d Orbital:** Ten electrons filling five boxes, all paired with opposing spins. - **5s Orbital:** One electron. ### Sections Describing Violations: 1. **Aufbau Violation:** - An empty box to describe potential configurations that violate the Aufbau Principle, which states that electrons fill the lowest energy orbitals first. 2. **Hund Violation:** - An empty box for potential violations of Hund's Rule, which states that electrons will fill degenerate orbitals singly first, with parallel spins, before pairing begins. 3. **Pauli Violation:** - An empty box to address configurations that might violate the Pauli Exclusion Principle, stating that no two electrons in the same atom can have the same four quantum numbers. These diagrams and sections are useful for teaching the correct electron configurations and identifying potential violations of fundamental principles in quantum chemistry.
Transcribed Image Text:The image displays diagrams illustrating electron configurations and potential violations of electron filling principles. ### Electron Configurations: 1. **First Diagram:** - **2s Orbital:** Two electrons with opposing spins. - **2p Orbital:** Three electrons with parallel spins in separate boxes. 2. **Second Diagram:** - **2s Orbital:** One electron. - **2p Orbital:** Three electrons with parallel spins in separate boxes. 3. **Third Diagram:** - **3s Orbital:** Two electrons with opposing spins. - **3p Orbital:** Three electrons, one pair with opposing spins and one single electron. 4. **Fourth Diagram:** - **4d Orbital:** Five electrons, three pairs and one single electron, with opposing spins depicted. - **5s Orbital:** Two electrons with opposing spins. 5. **Fifth Diagram:** - **4s Orbital:** Two electrons with opposing spins. - **3d Orbital:** Ten electrons filling five boxes, all paired with opposing spins. - **5s Orbital:** One electron. ### Sections Describing Violations: 1. **Aufbau Violation:** - An empty box to describe potential configurations that violate the Aufbau Principle, which states that electrons fill the lowest energy orbitals first. 2. **Hund Violation:** - An empty box for potential violations of Hund's Rule, which states that electrons will fill degenerate orbitals singly first, with parallel spins, before pairing begins. 3. **Pauli Violation:** - An empty box to address configurations that might violate the Pauli Exclusion Principle, stating that no two electrons in the same atom can have the same four quantum numbers. These diagrams and sections are useful for teaching the correct electron configurations and identifying potential violations of fundamental principles in quantum chemistry.
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