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How could we use the Bohr models to further elaborate the question about ionic bonds? Cite evidence from the image.

How could we use the Bohr models to further elaborate the question about ionic bonds? Cite evidence from the image.

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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How could we use the Bohr models to further elaborate the question about ionic bonds? Cite evidence from the image.

### Explaining Ionic Bonding with Sodium and Chlorine **Diagram Description:** This image illustrates the process of ionic bonding between sodium (Na) and chlorine (Cl) atoms. 1. **Initial State:** - **Sodium (Na) Atom:** - The sodium atom is represented with three concentric circles, indicating its electron shells. - The inner and second shells are filled, and the outermost shell has one electron (depicted in blue). - **Chlorine (Cl) Atom:** - The chlorine atom is shown with three concentric circles. - The inner two shells are filled, while the outermost shell has seven electrons (depicted in green). - An arrow indicates the transfer of the outermost electron from sodium to chlorine. 2. **Ionic Bond Formation:** - **Sodium Ion (Na⁺):** - After losing its outer electron, sodium becomes positively charged (Na⁺) and has a full outer shell. - **Chloride Ion (Cl⁻):** - Chlorine gains an electron, resulting in a negatively charged ion (Cl⁻) with a complete outer shell. - The purple background highlights the formation of an "ionic bond," where the oppositely charged ions attract each other, creating a stable compound. This diagram effectively demonstrates how the transfer of electrons leads to the formation of ions and the ionic bond, a fundamental concept in chemistry.
Transcribed Image Text:### Explaining Ionic Bonding with Sodium and Chlorine **Diagram Description:** This image illustrates the process of ionic bonding between sodium (Na) and chlorine (Cl) atoms. 1. **Initial State:** - **Sodium (Na) Atom:** - The sodium atom is represented with three concentric circles, indicating its electron shells. - The inner and second shells are filled, and the outermost shell has one electron (depicted in blue). - **Chlorine (Cl) Atom:** - The chlorine atom is shown with three concentric circles. - The inner two shells are filled, while the outermost shell has seven electrons (depicted in green). - An arrow indicates the transfer of the outermost electron from sodium to chlorine. 2. **Ionic Bond Formation:** - **Sodium Ion (Na⁺):** - After losing its outer electron, sodium becomes positively charged (Na⁺) and has a full outer shell. - **Chloride Ion (Cl⁻):** - Chlorine gains an electron, resulting in a negatively charged ion (Cl⁻) with a complete outer shell. - The purple background highlights the formation of an "ionic bond," where the oppositely charged ions attract each other, creating a stable compound. This diagram effectively demonstrates how the transfer of electrons leads to the formation of ions and the ionic bond, a fundamental concept in chemistry.
### What Types of Elements Form Ionic Bonds and Why? **Understanding Ionic Bonds:** Ionic bonds are a type of chemical bond that occurs between metals and nonmetals. These bonds form through the complete transfer of valence electrons from one atom to another. **The Role of the Octet Rule:** The process of ionic bonding is driven by the Octet Rule, which suggests that atoms are most stable when they have eight electrons in their valence shell. As mentioned in the text: - An atom can satisfy the Octet Rule by transferring valence electrons from one atom to another. **Formation of Ionic Bonds:** To achieve stability via the Octet Rule, a metal atom will donate its valence electrons to a nonmetal atom. Through this electron transfer, the metal becomes a positively charged ion, while the nonmetal becomes a negatively charged ion. The opposite charges attract, resulting in the formation of an ionic bond.
Transcribed Image Text:### What Types of Elements Form Ionic Bonds and Why? **Understanding Ionic Bonds:** Ionic bonds are a type of chemical bond that occurs between metals and nonmetals. These bonds form through the complete transfer of valence electrons from one atom to another. **The Role of the Octet Rule:** The process of ionic bonding is driven by the Octet Rule, which suggests that atoms are most stable when they have eight electrons in their valence shell. As mentioned in the text: - An atom can satisfy the Octet Rule by transferring valence electrons from one atom to another. **Formation of Ionic Bonds:** To achieve stability via the Octet Rule, a metal atom will donate its valence electrons to a nonmetal atom. Through this electron transfer, the metal becomes a positively charged ion, while the nonmetal becomes a negatively charged ion. The opposite charges attract, resulting in the formation of an ionic bond.
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