How many electrons can be described by the quantum numbers n=2, l=2, m=0. O 1 O 3 O 6 2.

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...
icon
Related questions
icon
Concept explainers
Question

28

**Title: Quantum Numbers and Electron Configuration**

**Question:**
How many electrons can be described by the quantum numbers \( n=2, l=2, m_l=0 \)?

**Options:**
- 1
- 3
- 6
- 0
- 2

**Explanation:**
To determine how many electrons can be described by the given quantum numbers \( n=2, l=2, m_l=0 \), we need to understand the meaning and restrictions of each quantum number:

1. **Principal Quantum Number (\(n\))**: Indicates the main energy level. \( n = 2 \) refers to the second energy level.
2. **Azimuthal Quantum Number (\(l\))**: Represents the subshell (or angular momentum). \( l = 2 \) corresponds to the \(d\)-subshell.
3. **Magnetic Quantum Number (\(m_l\))**: Specifies the orientation of the orbital. \( m_l = 0 \) means the orbital is oriented in a specific way in the magnetic field.

For given \( n \) and \( l \):
- \( n = 2 \)
- \( l = 2 \) (which is typically associated with the third principal quantum number. It seems there is probably a misunderstanding. The maximum \( l \) value for \( n=2 \) should be \( l=1 \), which corresponds to the \( p \)-subshell. However, assuming the context is set for advanced cases: assuming \( n=2 \), and considering \( l=2 \), then \( n \) should at least be 3 for \( l=2 \)).

Given \( m_l = 0 \), each orientation (each \( m_l \) value) can hold one electron with each of the two possible spin states (\( m_s = +\frac{1}{2} \) and \( m_s = -\frac{1}{2} \)).

Therefore, the answer is **2 electrons**: one for each possible spin state in the orbital described by \( n=2, l=2, m_l=0 \).

**Correct Answer:**
- 2
Transcribed Image Text:**Title: Quantum Numbers and Electron Configuration** **Question:** How many electrons can be described by the quantum numbers \( n=2, l=2, m_l=0 \)? **Options:** - 1 - 3 - 6 - 0 - 2 **Explanation:** To determine how many electrons can be described by the given quantum numbers \( n=2, l=2, m_l=0 \), we need to understand the meaning and restrictions of each quantum number: 1. **Principal Quantum Number (\(n\))**: Indicates the main energy level. \( n = 2 \) refers to the second energy level. 2. **Azimuthal Quantum Number (\(l\))**: Represents the subshell (or angular momentum). \( l = 2 \) corresponds to the \(d\)-subshell. 3. **Magnetic Quantum Number (\(m_l\))**: Specifies the orientation of the orbital. \( m_l = 0 \) means the orbital is oriented in a specific way in the magnetic field. For given \( n \) and \( l \): - \( n = 2 \) - \( l = 2 \) (which is typically associated with the third principal quantum number. It seems there is probably a misunderstanding. The maximum \( l \) value for \( n=2 \) should be \( l=1 \), which corresponds to the \( p \)-subshell. However, assuming the context is set for advanced cases: assuming \( n=2 \), and considering \( l=2 \), then \( n \) should at least be 3 for \( l=2 \)). Given \( m_l = 0 \), each orientation (each \( m_l \) value) can hold one electron with each of the two possible spin states (\( m_s = +\frac{1}{2} \) and \( m_s = -\frac{1}{2} \)). Therefore, the answer is **2 electrons**: one for each possible spin state in the orbital described by \( n=2, l=2, m_l=0 \). **Correct Answer:** - 2
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

Blurred answer
Knowledge Booster
Lipids
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY