A monatomic ion with a charge of +1 has an electronic configuration of 1s²2s²2p°3s²3p°. This ion is a(n) | It has the same electron configuration as the noble gas The symbol for the ion is:
A monatomic ion with a charge of +1 has an electronic configuration of 1s²2s²2p°3s²3p°. This ion is a(n) | It has the same electron configuration as the noble gas The symbol for the ion is:
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
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![### Understanding Electron Configuration and Ion Formation
**Concept: Monatomic Ions and Electron Configuration**
A monatomic ion with a charge of +1 has an electronic configuration of \(1s^2 2s^2 2p^6 3s^2 3p^6\).
**Questions and Answers:**
1. **Identify the Ion:**
- This ion is a(n) [text box/dropdown].
2. **Electron Configuration Comparison:**
- It has the same electron configuration as the noble gas [text box].
3. **Ion Symbol:**
- The symbol for the ion is: [text box].
**Explanation:**
The given electronic configuration corresponds to 18 electrons (2 in 1s, 2 in 2s, 6 in 2p, 2 in 3s, and 6 in 3p). For a neutral atom, this configuration corresponds to Argon (Ar). However, since the ion has a +1 charge, it means the neutral atom had 19 electrons before losing one to become the ion. Therefore, this ion is a Potassium ion (K⁺).
- **This ion is a K⁺.**
- **It has the same electron configuration as the noble gas Argon.**
- **The symbol for the ion is K⁺.**
This educational exercise helps in understanding the relationship between electron configuration, ions, and their corresponding noble gases.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1f61489d-b599-4717-b8e4-1c0e8dbf11ad%2F8cf28a74-e08d-42cb-9e1a-79684cc765e9%2Fbxano5.png&w=3840&q=75)
Transcribed Image Text:### Understanding Electron Configuration and Ion Formation
**Concept: Monatomic Ions and Electron Configuration**
A monatomic ion with a charge of +1 has an electronic configuration of \(1s^2 2s^2 2p^6 3s^2 3p^6\).
**Questions and Answers:**
1. **Identify the Ion:**
- This ion is a(n) [text box/dropdown].
2. **Electron Configuration Comparison:**
- It has the same electron configuration as the noble gas [text box].
3. **Ion Symbol:**
- The symbol for the ion is: [text box].
**Explanation:**
The given electronic configuration corresponds to 18 electrons (2 in 1s, 2 in 2s, 6 in 2p, 2 in 3s, and 6 in 3p). For a neutral atom, this configuration corresponds to Argon (Ar). However, since the ion has a +1 charge, it means the neutral atom had 19 electrons before losing one to become the ion. Therefore, this ion is a Potassium ion (K⁺).
- **This ion is a K⁺.**
- **It has the same electron configuration as the noble gas Argon.**
- **The symbol for the ion is K⁺.**
This educational exercise helps in understanding the relationship between electron configuration, ions, and their corresponding noble gases.
![### Understanding Electron Configuration for Sulfur Ion
**Problem Statement:**
Assuming that the octet rule is obeyed, write out the electron configuration for the ion formed by the element sulfur (S).
**Electron Configuration:**
The electron configuration for sulfur is:
\[ 1s^2 2s^2 2p^6 3s^2 3p^4 \]
**Ion Formation:**
- This ion is a(n) **anion** with a charge of **2⁻**.
- When sulfur gains 2 electrons to form an anion (S²⁻), its electron configuration becomes:
\[ 1s^2 2s^2 2p^6 3s^2 3p^6 \]
Thus, it achieves the same electron configuration as the noble gas **argon (Ar)**.
### Explanation
Sulfur, with an atomic number of 16, has 16 electrons when neutral. The electron configuration reflects the distribution of these electrons in the different energy levels. By gaining 2 electrons to form an S²⁻ ion, sulfur reaches a stable electron arrangement similar to that of the noble gas argon, which has a full valence shell with 18 electrons. This configuration is more stable due to having a complete octet in its outermost shell.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1f61489d-b599-4717-b8e4-1c0e8dbf11ad%2F8cf28a74-e08d-42cb-9e1a-79684cc765e9%2Fcvr1f67.png&w=3840&q=75)
Transcribed Image Text:### Understanding Electron Configuration for Sulfur Ion
**Problem Statement:**
Assuming that the octet rule is obeyed, write out the electron configuration for the ion formed by the element sulfur (S).
**Electron Configuration:**
The electron configuration for sulfur is:
\[ 1s^2 2s^2 2p^6 3s^2 3p^4 \]
**Ion Formation:**
- This ion is a(n) **anion** with a charge of **2⁻**.
- When sulfur gains 2 electrons to form an anion (S²⁻), its electron configuration becomes:
\[ 1s^2 2s^2 2p^6 3s^2 3p^6 \]
Thus, it achieves the same electron configuration as the noble gas **argon (Ar)**.
### Explanation
Sulfur, with an atomic number of 16, has 16 electrons when neutral. The electron configuration reflects the distribution of these electrons in the different energy levels. By gaining 2 electrons to form an S²⁻ ion, sulfur reaches a stable electron arrangement similar to that of the noble gas argon, which has a full valence shell with 18 electrons. This configuration is more stable due to having a complete octet in its outermost shell.
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