D Incorrect 3p n = 3 3p l = 0 Incorrect The possible values of me for the 3p subshell are -2, -1,0, +1, +2 -1,0, +1 Incorrect 0 -3, -2,-1, 0, +1, +2, +3
D Incorrect 3p n = 3 3p l = 0 Incorrect The possible values of me for the 3p subshell are -2, -1,0, +1, +2 -1,0, +1 Incorrect 0 -3, -2,-1, 0, +1, +2, +3
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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Atomic Structure
The basic structure of an atom is defined as the component-level of atomic structure of an atom. Precisely speaking an atom consists of three major subatomic particles which are protons, neutrons, and electrons. Many theories have been stated for explaining the structure of an atom.
Shape of the D Orbital
Shapes of orbitals are an approximate representation of boundaries in space for finding electrons occupied in that respective orbital. D orbitals are known to have a clover leaf shape or dumbbell inside where electrons can be found.
Question
![### Quantum Numbers for the 3p Subshell
**Incorrect Inputs:**
1. **Principal Quantum Number (\( n \)) for 3p**:
\[
3p \quad n = 3
\]
*Result: Incorrect*
2. **Azimuthal Quantum Number (\( \ell \)) for 3p**:
\[
3p \quad \ell = 0
\]
*Result: Incorrect*
**Question:**
The possible values of magnetic quantum number (\( m_\ell \)) for the 3p subshell are:
- \(-2, -1, 0, +1, +2\)
- \(-1, 0, +1\)
- \(0\)
- \(-3, -2, -1, 0, +1, +2, +3\)
*A selection was made for option "0" which is incorrect.*
**Explanation:**
For a 3p subshell:
- The principal quantum number (\( n \)) is correctly \(3\).
- The azimuthal quantum number (\( \ell \)) for a 'p' orbital is \(1\), not \(0\).
- The magnetic quantum number (\( m_\ell \)) can have values from \(-\ell\) to \(+\ell\), which are \(-1, 0, +1\) for a p orbital.
Correct responses are critical for understanding the electronic configuration of atoms.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F87c9e35a-c40b-4293-8ffa-6a1a5ded8456%2F1f46058c-78d2-440f-80eb-5152d208e990%2F71clb4l_processed.png&w=3840&q=75)
Transcribed Image Text:### Quantum Numbers for the 3p Subshell
**Incorrect Inputs:**
1. **Principal Quantum Number (\( n \)) for 3p**:
\[
3p \quad n = 3
\]
*Result: Incorrect*
2. **Azimuthal Quantum Number (\( \ell \)) for 3p**:
\[
3p \quad \ell = 0
\]
*Result: Incorrect*
**Question:**
The possible values of magnetic quantum number (\( m_\ell \)) for the 3p subshell are:
- \(-2, -1, 0, +1, +2\)
- \(-1, 0, +1\)
- \(0\)
- \(-3, -2, -1, 0, +1, +2, +3\)
*A selection was made for option "0" which is incorrect.*
**Explanation:**
For a 3p subshell:
- The principal quantum number (\( n \)) is correctly \(3\).
- The azimuthal quantum number (\( \ell \)) for a 'p' orbital is \(1\), not \(0\).
- The magnetic quantum number (\( m_\ell \)) can have values from \(-\ell\) to \(+\ell\), which are \(-1, 0, +1\) for a p orbital.
Correct responses are critical for understanding the electronic configuration of atoms.
![### Quantum Numbers and Electron Configuration
#### Chemical Symbol Determination
Give the chemical symbol for the element with the ground-state electron configuration \([Ne]3s^23p^2\).
- **Symbol:**
- Input: 0
- **Status:** Incorrect
#### Quantum Numbers Analysis
Determine the quantum numbers \( n \) and \( \ell \) and select all possible values for \( m_\ell \) for each subshell of the element.
- **For \( 3s \) subshell:**
- \( n = \)
- Input: 1
- **Status:** Incorrect
- \( \ell = \)
- Input: 2
- **Status:** Incorrect
#### \( m_\ell \) Values Selection
The possible values of \( m_\ell \) for the \( 3s \) subshell are:
- Options:
- \((-1, 0, +1)\)
- \((-3, -2, -1, 0, +1, +2, +3)\)
- \((-2, -1, 0, +1, +2)\)
- \(0\) (Selected)
The selection is incorrect based on the context of the \( 3s \) subshell, where only the value \(0\) is applicable as \( m_\ell \) is determined by \(\ell = 0\).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F87c9e35a-c40b-4293-8ffa-6a1a5ded8456%2F1f46058c-78d2-440f-80eb-5152d208e990%2Fs0ly0gi_processed.png&w=3840&q=75)
Transcribed Image Text:### Quantum Numbers and Electron Configuration
#### Chemical Symbol Determination
Give the chemical symbol for the element with the ground-state electron configuration \([Ne]3s^23p^2\).
- **Symbol:**
- Input: 0
- **Status:** Incorrect
#### Quantum Numbers Analysis
Determine the quantum numbers \( n \) and \( \ell \) and select all possible values for \( m_\ell \) for each subshell of the element.
- **For \( 3s \) subshell:**
- \( n = \)
- Input: 1
- **Status:** Incorrect
- \( \ell = \)
- Input: 2
- **Status:** Incorrect
#### \( m_\ell \) Values Selection
The possible values of \( m_\ell \) for the \( 3s \) subshell are:
- Options:
- \((-1, 0, +1)\)
- \((-3, -2, -1, 0, +1, +2, +3)\)
- \((-2, -1, 0, +1, +2)\)
- \(0\) (Selected)
The selection is incorrect based on the context of the \( 3s \) subshell, where only the value \(0\) is applicable as \( m_\ell \) is determined by \(\ell = 0\).
Expert Solution
Step 1
n standard for principle quantum number
l standards for azimuthal quantum number
ml stands for magnetic quantum number
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