18. Which orbital diagram(s) in Figure P7.8 represent:(a) the ground state of an oxygen cation, O⁺?(b) an excited state of a nitrogen atom?(c) a violation of Hund's rule? This image depicts four different electron configurations labeled (a), (b), (c), and (d). The diagrams illustrate how electrons fill the atomic orbitals for an atom.Each configuration consists of three sets of boxes representing atomic orbitals: the 1s, 2s, and 2p orbitals. Each box within these orbitals symbolically represents an electron's spin state using an arrow. An upward arrow indicates a positive spin (+1/2), while a downward arrow indicates a negative spin (-1/2).1. **Configuration (a):** - **1s orbital:** Contains one pair of electrons with opposite spins (represented by one upward and one downward arrow). - **2s orbital:** Contains one pair of electrons with opposite spins. - **2p orbital:** Contains one electron with an upward spin in the first box and one electron with a downward spin in the second box. The third box is empty.2. **Configuration (b):** - **1s orbital:** Contains one pair of electrons with opposite spins. - **2s orbital:** Contains one electron with an upward spin. - **2p orbital:** Each box contains one electron with upward spins, indicating the filling of each sub-orbital in 2p according to Hund's rule, which states that every orbital in a subshell gets one electron before any orbital gets a second.3. **Configuration (c):** - **1s orbital:** Contains one pair of electrons with opposite spins. - **2s orbital:** Contains one electron with an upward spin. - **2p orbital:** The first box contains a pair of electrons with opposite spins. The second box has one electron with an upward spin, and the third box also has one electron with an upward spin.4. **Configuration (d):** - **1s orbital:** Contains one pair of electrons with opposite spins. - **2s orbital:** Contains one pair of electrons. - **2p orbital:** The first box contains one pair of electrons with opposite spins. The second box has one electron with an upward spin, and the third box is empty.These electron configurations depict different filling sequences and are useful for understanding the electronic structure of atoms, especially in terms of Hund's Rule and the Pauli Exclusion Principle guiding electron arrangements in orbitals.

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Answered: 18. Which orbital diagram(s) in Figure…

18. Which orbital diagram(s) in Figure P7.8 represent: (a) the ground state of an oxygen cation, O+? (b) an excited state of a nitrogen atom? (c) a violation of Hund's rule?

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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Question

18. Which orbital diagram(s) in Figure P7.8 represent:
(a) the ground state of an oxygen cation, O⁺?
(b) an excited state of a nitrogen atom?
(c) a violation of Hund's rule?

This image depicts four different electron configurations labeled (a), (b), (c), and (d). The diagrams illustrate how electrons fill the atomic orbitals for an atom.

Each configuration consists of three sets of boxes representing atomic orbitals: the 1s, 2s, and 2p orbitals. Each box within these orbitals symbolically represents an electron's spin state using an arrow. An upward arrow indicates a positive spin (+1/2), while a downward arrow indicates a negative spin (-1/2).

1. **Configuration (a):**
- **1s orbital:** Contains one pair of electrons with opposite spins (represented by one upward and one downward arrow).
- **2s orbital:** Contains one pair of electrons with opposite spins.
- **2p orbital:** Contains one electron with an upward spin in the first box and one electron with a downward spin in the second box. The third box is empty.

2. **Configuration (b):**
- **1s orbital:** Contains one pair of electrons with opposite spins.
- **2s orbital:** Contains one electron with an upward spin.
- **2p orbital:** Each box contains one electron with upward spins, indicating the filling of each sub-orbital in 2p according to Hund's rule, which states that every orbital in a subshell gets one electron before any orbital gets a second.

3. **Configuration (c):**
- **1s orbital:** Contains one pair of electrons with opposite spins.
- **2s orbital:** Contains one electron with an upward spin.
- **2p orbital:** The first box contains a pair of electrons with opposite spins. The second box has one electron with an upward spin, and the third box also has one electron with an upward spin.

4. **Configuration (d):**
- **1s orbital:** Contains one pair of electrons with opposite spins.
- **2s orbital:** Contains one pair of electrons.
- **2p orbital:** The first box contains one pair of electrons with opposite spins. The second box has one electron with an upward spin, and the third box is empty.

These electron configurations depict different filling sequences and are useful for understanding the electronic structure of atoms, especially in terms of Hund's Rule and the Pauli Exclusion Principle guiding electron arrangements in orbitals.

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