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CREATE A CEPT MAP FROM THIS PASSAGE: In this article, we will discuss polyatomic ions. The prefix poly means many, so a polyatomic ion is an ion that contains more than one atom. This differentiates polyatomic ions from monatomic ions, which contain only one atom. Examples of monatomic ions include Na¹, Fe, Cl and many, many others. We can think about polyatomic ions by comparing them to monatomic ions. A monatomic ion is an atom that has been ionized by gaining or losing electrons. The ion has a net charge because the total number of electrons is not balanced by the total number of protons in the nucleus. Thus, compared to the neutral atom, we have extra electrons-in the case of a negatively charged anion-or not enough electrons-in the case of a positively charged cation. Similarly, we can think of a polyatomic ion as a molecule that has been ionized by gaining or losing electrons. In a polyatomic ion, the group of covalently bonded atoms carries a net charge because the total number of electrons in the molecule is not equal to the total number of protons in the molecule. Examples of polyatomic ions include NH, CO,2, PO,, and many others.

CREATE A CEPT MAP FROM THIS PASSAGE: In this article, we will discuss polyatomic ions. The prefix poly means many, so a polyatomic ion is an ion that contains more than one atom. This differentiates polyatomic ions from monatomic ions, which contain only one atom. Examples of monatomic ions include Na¹, Fe, Cl and many, many others. We can think about polyatomic ions by comparing them to monatomic ions. A monatomic ion is an atom that has been ionized by gaining or losing electrons. The ion has a net charge because the total number of electrons is not balanced by the total number of protons in the nucleus. Thus, compared to the neutral atom, we have extra electrons-in the case of a negatively charged anion-or not enough electrons-in the case of a positively charged cation. Similarly, we can think of a polyatomic ion as a molecule that has been ionized by gaining or losing electrons. In a polyatomic ion, the group of covalently bonded atoms carries a net charge because the total number of electrons in the molecule is not equal to the total number of protons in the molecule. Examples of polyatomic ions include NH, CO,2, PO,, and many others.

Chemistry
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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Create a concept map from the passage attached. Add personalization. Example of a concept map is attached.

**Create a Concept Map from this Passage:** In this article, we will discuss polyatomic ions. The prefix *poly-* means many, so a polyatomic ion is an ion that contains more than one atom. This differentiates polyatomic ions from monatomic ions, which contain only one atom. Examples of monatomic ions include Na⁺¹, Fe³⁺, Cl⁻¹, and many others. We can think about polyatomic ions by comparing them to monatomic ions. A monatomic ion is an atom that has been ionized by gaining or losing electrons. The ion has a net charge because the total number of electrons is not balanced by the total number of protons in the nucleus. Thus, compared to the neutral atom, we have extra electrons—in the case of a negatively charged anion—or not enough electrons—in the case of a positively charged cation. Similarly, we can think of a polyatomic ion as a molecule that has been ionized by gaining or losing electrons. In a polyatomic ion, the group of covalently bonded atoms carries a net charge because the total number of electrons in the molecule is not equal to the total number of protons in the molecule. Examples of polyatomic ions include NH₄⁺, CO₃²⁻, PO₄³⁻, and many others.
Transcribed Image Text:**Create a Concept Map from this Passage:** In this article, we will discuss polyatomic ions. The prefix *poly-* means many, so a polyatomic ion is an ion that contains more than one atom. This differentiates polyatomic ions from monatomic ions, which contain only one atom. Examples of monatomic ions include Na⁺¹, Fe³⁺, Cl⁻¹, and many others. We can think about polyatomic ions by comparing them to monatomic ions. A monatomic ion is an atom that has been ionized by gaining or losing electrons. The ion has a net charge because the total number of electrons is not balanced by the total number of protons in the nucleus. Thus, compared to the neutral atom, we have extra electrons—in the case of a negatively charged anion—or not enough electrons—in the case of a positively charged cation. Similarly, we can think of a polyatomic ion as a molecule that has been ionized by gaining or losing electrons. In a polyatomic ion, the group of covalently bonded atoms carries a net charge because the total number of electrons in the molecule is not equal to the total number of protons in the molecule. Examples of polyatomic ions include NH₄⁺, CO₃²⁻, PO₄³⁻, and many others.
### Understanding the Octet Rule and Atomic Stability The **Octet Rule** explains the tendency of atoms to achieve a stable electron configuration, akin to noble gases, by having eight valence electrons. This principle is critical to understanding chemical reactions and bonding. **Key Concepts:** 1. **Electron Behavior:** - Atoms react by gaining or losing electrons from their valence orbitals. - **Gain of Electrons**: Leads to the formation of anions (negative ions). - **Loss of Electrons**: Results in the formation of cations (positive ions). 2. **Bond Formation:** - **Ionic Bonds**: Formed by the transfer of electrons between metals and nonmetals. - **Covalent Bonds**: Result from the sharing of electrons. 3. **Atomic Interactions:** - Metals tend to lose electrons to form cations. - Nonmetals typically gain electrons to form anions. 4. **Stability and Configuration:** - Atoms that achieve eight valence electrons attain a stable electronic configuration. - Noble gases (except helium) inherently have a full octet, serving as models of stability. 5. **Historical Context:** - The octet rule was discovered by Walther Kossel and Gilbert Newton Lewis. This framework aids in comprehending how atoms interact and how stable compounds form through achieving a full octet of electrons. Understanding these principles is crucial for studying chemical reactions and predicting molecular structures.
Transcribed Image Text:### Understanding the Octet Rule and Atomic Stability The **Octet Rule** explains the tendency of atoms to achieve a stable electron configuration, akin to noble gases, by having eight valence electrons. This principle is critical to understanding chemical reactions and bonding. **Key Concepts:** 1. **Electron Behavior:** - Atoms react by gaining or losing electrons from their valence orbitals. - **Gain of Electrons**: Leads to the formation of anions (negative ions). - **Loss of Electrons**: Results in the formation of cations (positive ions). 2. **Bond Formation:** - **Ionic Bonds**: Formed by the transfer of electrons between metals and nonmetals. - **Covalent Bonds**: Result from the sharing of electrons. 3. **Atomic Interactions:** - Metals tend to lose electrons to form cations. - Nonmetals typically gain electrons to form anions. 4. **Stability and Configuration:** - Atoms that achieve eight valence electrons attain a stable electronic configuration. - Noble gases (except helium) inherently have a full octet, serving as models of stability. 5. **Historical Context:** - The octet rule was discovered by Walther Kossel and Gilbert Newton Lewis. This framework aids in comprehending how atoms interact and how stable compounds form through achieving a full octet of electrons. Understanding these principles is crucial for studying chemical reactions and predicting molecular structures.
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