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3. Is this arrangement of electrons possible, why or why not? 4. What would happen, eventually, to the electron in the highest energy level in Model 1? 5. Write the electronic configuration corresponding to the electronic arrangement 6. Write out the ground state electron configuration for this atom.

3. Is this arrangement of electrons possible, why or why not? 4. What would happen, eventually, to the electron in the highest energy level in Model 1? 5. Write the electronic configuration corresponding to the electronic arrangement 6. Write out the ground state electron configuration for this atom.

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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3. Is this arrangement of electrons possible, why or why not?

4. What would happen, eventually, to the electron in the highest energy level in Model 1?

5. Write the electronic configuration corresponding to the electronic arrangement

6. Write out the ground state electron configuration for this atom.

The image illustrates electron configurations in various atomic orbitals through an orbital diagram. Here is a detailed transcription and explanation: ### Orbital Diagram Explanation 1. **1s Orbital:** - Contains one box labeled "1s." - Two arrows inside the box; one arrow pointing upwards and one pointing downwards, indicating the presence of two electrons with opposite spins. This configuration shows a filled 1s orbital. 2. **2s Orbital:** - Contains one box labeled "2s." - Two arrows are inside the box; one pointing upwards and one pointing downwards, indicating a filled 2s orbital with two electrons of opposite spins. 3. **2p Orbitals:** - Contains three boxes labeled "2p." - The first box contains two arrows (one up, one down), indicating a filled orbital. - The second box contains one downward arrow, indicating an orbital with one electron. - The third box contains two arrows (one up, one down), indicating a filled orbital. - This configuration illustrates the distribution of electrons in a 2p subshell according to Hund's rule. 4. **3s Orbital:** - Contains one empty box labeled "3s." - The "3s" orbital does not have any electrons based on this diagram. 5. **3p Orbitals:** - Contains three boxes labeled "3p." - The first box contains one upward arrow, indicating it contains one electron. - The second and third boxes are empty, indicating they do not have electrons. ### Diagram Explanation - Each box represents an atomic orbital. - Arrows within boxes indicate electrons; the direction of the arrow (up or down) represents the spin of the electron. - Configurations follow the Aufbau principle, Pauli exclusion principle, and Hund's rule. This diagram displays electron configurations typically taught in chemistry education for illustrating atomic structure and behavior.
Transcribed Image Text:The image illustrates electron configurations in various atomic orbitals through an orbital diagram. Here is a detailed transcription and explanation: ### Orbital Diagram Explanation 1. **1s Orbital:** - Contains one box labeled "1s." - Two arrows inside the box; one arrow pointing upwards and one pointing downwards, indicating the presence of two electrons with opposite spins. This configuration shows a filled 1s orbital. 2. **2s Orbital:** - Contains one box labeled "2s." - Two arrows are inside the box; one pointing upwards and one pointing downwards, indicating a filled 2s orbital with two electrons of opposite spins. 3. **2p Orbitals:** - Contains three boxes labeled "2p." - The first box contains two arrows (one up, one down), indicating a filled orbital. - The second box contains one downward arrow, indicating an orbital with one electron. - The third box contains two arrows (one up, one down), indicating a filled orbital. - This configuration illustrates the distribution of electrons in a 2p subshell according to Hund's rule. 4. **3s Orbital:** - Contains one empty box labeled "3s." - The "3s" orbital does not have any electrons based on this diagram. 5. **3p Orbitals:** - Contains three boxes labeled "3p." - The first box contains one upward arrow, indicating it contains one electron. - The second and third boxes are empty, indicating they do not have electrons. ### Diagram Explanation - Each box represents an atomic orbital. - Arrows within boxes indicate electrons; the direction of the arrow (up or down) represents the spin of the electron. - Configurations follow the Aufbau principle, Pauli exclusion principle, and Hund's rule. This diagram displays electron configurations typically taught in chemistry education for illustrating atomic structure and behavior.
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