Provide the quantum numbers and related information for the following orbital, 3d. What is the maximum number of electrons in the entire shell?
Provide the quantum numbers and related information for the following orbital, 3d. What is the maximum number of electrons in the entire shell?
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
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![**Question: Quantum Numbers and Electron Capacity**
**Task:**
Provide the quantum numbers and related information for the following orbital, 3d.
What is the maximum number of electrons in the entire shell?
**Explanation:**
Quantum numbers describe the properties of atomic orbitals and the properties of electrons in orbitals. Here is a breakdown for the 3d orbital:
- **Principal Quantum Number (n):** 3
- This number indicates the main energy level occupied by the electron.
- **Azimuthal Quantum Number (l):** 2
- Corresponds to the d subshell (l = 0 for s, 1 for p, 2 for d, 3 for f).
- **Magnetic Quantum Number (mᵢ):** -2, -1, 0, 1, 2
- These numbers describe the orientation of the orbital in space.
- **Spin Quantum Number (s):** +1/2 or -1/2
- Indicates the two possible orientations of the electron’s spin.
**Maximum Number of Electrons:**
Each d orbital can hold a maximum of 2 electrons. Since there are 5 orbitals in the d subshell (corresponding to mᵢ values), the maximum number of electrons in a 3d subshell is:
\[ 5 \text{ orbitals} \times 2 \text{ electrons/orbital} = 10 \text{ electrons} \]
For the entire n=3 shell, including the 3s, 3p, and 3d subshells:
- 3s subshell: 1 orbital (2 electrons)
- 3p subshell: 3 orbitals (6 electrons)
- 3d subshell: 5 orbitals (10 electrons)
So the maximum number of electrons in the n=3 shell is:
\[ 2 (3s) + 6 (3p) + 10 (3d) = 18 \text{ electrons} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4bb26d64-bb49-4ec5-afc7-ea9f4d31dfb0%2Fee1eee6a-f41d-4033-affa-0242888919f2%2Fkup72qm_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question: Quantum Numbers and Electron Capacity**
**Task:**
Provide the quantum numbers and related information for the following orbital, 3d.
What is the maximum number of electrons in the entire shell?
**Explanation:**
Quantum numbers describe the properties of atomic orbitals and the properties of electrons in orbitals. Here is a breakdown for the 3d orbital:
- **Principal Quantum Number (n):** 3
- This number indicates the main energy level occupied by the electron.
- **Azimuthal Quantum Number (l):** 2
- Corresponds to the d subshell (l = 0 for s, 1 for p, 2 for d, 3 for f).
- **Magnetic Quantum Number (mᵢ):** -2, -1, 0, 1, 2
- These numbers describe the orientation of the orbital in space.
- **Spin Quantum Number (s):** +1/2 or -1/2
- Indicates the two possible orientations of the electron’s spin.
**Maximum Number of Electrons:**
Each d orbital can hold a maximum of 2 electrons. Since there are 5 orbitals in the d subshell (corresponding to mᵢ values), the maximum number of electrons in a 3d subshell is:
\[ 5 \text{ orbitals} \times 2 \text{ electrons/orbital} = 10 \text{ electrons} \]
For the entire n=3 shell, including the 3s, 3p, and 3d subshells:
- 3s subshell: 1 orbital (2 electrons)
- 3p subshell: 3 orbitals (6 electrons)
- 3d subshell: 5 orbitals (10 electrons)
So the maximum number of electrons in the n=3 shell is:
\[ 2 (3s) + 6 (3p) + 10 (3d) = 18 \text{ electrons} \]
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Transcribed Image Text:**Question 17.e of 24**
*Provide the quantum numbers and related information for the following orbital, 3d.*
**What is the maximum number of electrons in the entire shell?**
- *Incorrect, 1 attempt remaining*
*Your submitted answer contains too few significant figures.*
**Your submission:**
- 10 electrons
**Feedback:**
- *You have identified the number of electrons in the d orbital set alone. Recall that this question asks for the number of electrons in the entire n = 3 shell.*
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