---### Electronic Configuration and Isoelectronic Concepts#### Understanding Monatomic Ion Configuration**Problem Statement:**A monatomic ion with a charge of -1 has an electronic configuration of 1s² 2s² 2p⁶ 3s² 3p⁶.**Questions:**1. **This ion is a(n) _________.** 2. **What is the formula of the ion?**3. **What is the chemical symbol of the noble gas this ion is isoelectronic with?****Periodic Table Referenced:**On the right side of the page, a portion of the periodic table is shown. It highlights many elements along periods and groups. The elements are organized by increasing atomic number from left to right and top to bottom.**Answer and Explanation:**1. **This ion is a(n) __Chloride Ion (Cl⁻)__.**2. **What is the formula of the ion?** The formula is __Cl⁻__.3. **What is the chemical symbol of the noble gas this ion is isoelectronic with?** The ion Chloride (Cl⁻) is isoelectronic with the Noble Gas __Argon (Ar)__.**Explanation:**- A monatomic ion with a charge of -1 indicates that the element has gained one electron.- The electronic configuration given: 1s² 2s² 2p⁶ 3s² 3p⁶ matches the configuration of the noble gas Argon (Ar), which means they share the same number of electrons (18 electrons).- The ion is formed from an element in Group 17 of the periodic table (halogens) which typically form -1 anions. The element with the atomic number closest to Argon, which becomes Chloride (Cl) when gaining one electron.Using this periodic table diagram:![Periodic Table](https://links.to/periodic_table_image)It aids in identifying Chlorine as the nearest halogen to Argon when gaining an electron to form Cl⁻.---**Educational Note:**This type of problem helps in understanding how electronic configurations determine the identity of ions, and how to use the periodic table to find elements and their isoelectronic counterparts.---

If an atom gains one electron then it becomes X-1. Here, the configuration of Ion is 1s2 2s2 2p6 3s2…

Answered: This ion is a(n)

Science

Chemistry

This ion is a(n)

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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Question

---

### Electronic Configuration and Isoelectronic Concepts

#### Understanding Monatomic Ion Configuration

**Problem Statement:**

A monatomic ion with a charge of -1 has an electronic configuration of
1s² 2s² 2p⁶ 3s² 3p⁶.

**Questions:**

1. **This ion is a(n) _________.**

2. **What is the formula of the ion?**

3. **What is the chemical symbol of the noble gas this ion is isoelectronic with?**

**Periodic Table Referenced:**

On the right side of the page, a portion of the periodic table is shown. It highlights many elements along periods and groups. The elements are organized by increasing atomic number from left to right and top to bottom.

**Answer and Explanation:**

1. **This ion is a(n) __Chloride Ion (Cl⁻)__.**

2. **What is the formula of the ion?**
The formula is __Cl⁻__.

3. **What is the chemical symbol of the noble gas this ion is isoelectronic with?**
The ion Chloride (Cl⁻) is isoelectronic with the Noble Gas __Argon (Ar)__.

**Explanation:**

- A monatomic ion with a charge of -1 indicates that the element has gained one electron.
- The electronic configuration given: 1s² 2s² 2p⁶ 3s² 3p⁶ matches the configuration of the noble gas Argon (Ar), which means they share the same number of electrons (18 electrons).
- The ion is formed from an element in Group 17 of the periodic table (halogens) which typically form -1 anions. The element with the atomic number closest to Argon, which becomes Chloride (Cl) when gaining one electron.

Using this periodic table diagram:
![Periodic Table](https://links.to/periodic_table_image)

It aids in identifying Chlorine as the nearest halogen to Argon when gaining an electron to form Cl⁻.

---

**Educational Note:**
This type of problem helps in understanding how electronic configurations determine the identity of ions, and how to use the periodic table to find elements and their isoelectronic counterparts.

---

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