▼ ▼ Part B Calculate Zeff for the 4s electron in a copper atom, Cu. Express your answer numerically. ►View Available Hint(s) Zelf = Submit Part C Zelf= —| ΑΣΦ Calculate for a 3d electron in a copper atom, Cu. Express your answer numerically. View Available Hint(s) Submit h ΠΑΠΙ ΑΣΦ 3 → C ? ?
▼ ▼ Part B Calculate Zeff for the 4s electron in a copper atom, Cu. Express your answer numerically. ►View Available Hint(s) Zelf = Submit Part C Zelf= —| ΑΣΦ Calculate for a 3d electron in a copper atom, Cu. Express your answer numerically. View Available Hint(s) Submit h ΠΑΠΙ ΑΣΦ 3 → C ? ?
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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![Effective nuclear charge, \( Z_{\text{eff}} \), is defined as
\[
Z_{\text{eff}} = Z - S
\]
where \( Z \) is the true nuclear charge and \( S \) is the amount of shielding.
In 1930, John C. Slater devised the following set of empirical rules to estimate \( S \) for a designated \( ns \) or \( np \) electron:
i. Write the electron configuration of the element, and group the subshells as follows: \( (1s), (2s, 2p), (3s, 3p), (3d), (4s, 4p), (4d), (4f), (5s, 5p) \), and so on.
ii. Electrons in groups to the right of the \( (ns, np) \) group contribute nothing to the shielding constant for the designated electron.
iii. All the other electrons in the \( (ns, np) \) group shield the designated electron to the extent of 0.35 each.
iv. All electrons in the \( n-1 \) shell shield to the extent of 0.85 each.
v. All electrons in the \( n-2 \) shell, or lower, shield completely—their contributions to the shielding constant are 1.00 each.
When the designated electron is in an \( nd \) or \( nf \) group, rules (i), (ii), and (iii) remain the same but rules (iv) and (v) are replaced by the following:
vi. Each electron in a group lying to the left of the \( nd \) or \( nf \) group contributes 1.00 to the shielding constant.
These rules are a simplified generalization based on the average behavior of different types of electrons.
---
**Part A**
Calculate \( Z_{\text{eff}} \) for a valence electron in an oxygen atom.
Express your answer numerically:
\[
Z_{\text{eff}} =
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F77ff0dc1-7282-4fa0-94cd-a91857c24dd6%2F951e5a5d-d65b-4540-9729-4ba6d94245ff%2Ftvinzo7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Effective nuclear charge, \( Z_{\text{eff}} \), is defined as
\[
Z_{\text{eff}} = Z - S
\]
where \( Z \) is the true nuclear charge and \( S \) is the amount of shielding.
In 1930, John C. Slater devised the following set of empirical rules to estimate \( S \) for a designated \( ns \) or \( np \) electron:
i. Write the electron configuration of the element, and group the subshells as follows: \( (1s), (2s, 2p), (3s, 3p), (3d), (4s, 4p), (4d), (4f), (5s, 5p) \), and so on.
ii. Electrons in groups to the right of the \( (ns, np) \) group contribute nothing to the shielding constant for the designated electron.
iii. All the other electrons in the \( (ns, np) \) group shield the designated electron to the extent of 0.35 each.
iv. All electrons in the \( n-1 \) shell shield to the extent of 0.85 each.
v. All electrons in the \( n-2 \) shell, or lower, shield completely—their contributions to the shielding constant are 1.00 each.
When the designated electron is in an \( nd \) or \( nf \) group, rules (i), (ii), and (iii) remain the same but rules (iv) and (v) are replaced by the following:
vi. Each electron in a group lying to the left of the \( nd \) or \( nf \) group contributes 1.00 to the shielding constant.
These rules are a simplified generalization based on the average behavior of different types of electrons.
---
**Part A**
Calculate \( Z_{\text{eff}} \) for a valence electron in an oxygen atom.
Express your answer numerically:
\[
Z_{\text{eff}} =
\]
![**Part B**
Calculate \( Z_{\text{eff}} \) for the 4s electron in a copper atom, Cu.
Express your answer numerically.
[View Available Hint(s)]
Input box: \( Z_{\text{eff}} = \_\_\_ \)
[Submit button]
---
**Part C**
Calculate \( Z_{\text{eff}} \) for a 3d electron in a copper atom, Cu.
Express your answer numerically.
[View Available Hint(s)]
Input box: \( Z_{\text{eff}} = \_\_\_ \)
[Submit button]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F77ff0dc1-7282-4fa0-94cd-a91857c24dd6%2F951e5a5d-d65b-4540-9729-4ba6d94245ff%2F9bwb74_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Part B**
Calculate \( Z_{\text{eff}} \) for the 4s electron in a copper atom, Cu.
Express your answer numerically.
[View Available Hint(s)]
Input box: \( Z_{\text{eff}} = \_\_\_ \)
[Submit button]
---
**Part C**
Calculate \( Z_{\text{eff}} \) for a 3d electron in a copper atom, Cu.
Express your answer numerically.
[View Available Hint(s)]
Input box: \( Z_{\text{eff}} = \_\_\_ \)
[Submit button]
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