**Using Lewis Theory and Molecular Geometry**4. **Lewis Theory and Diatomic Nature of Nitrogen Gas** - Using Lewis theory, explain why nitrogen gas (N₂) exists as a diatomic molecule. Discuss the sharing of electrons and the formation of a triple bond between nitrogen atoms. Highlight the stability achieved through this configuration according to Lewis structures.5. **Molecular and Ion Structure Analysis** - For each molecule or ion, complete the following tasks: (a) **Determining Valence Electrons** - Calculate the total number of valence electrons available for bonding, as well as the electron pairs available for bonding. (b) **Drawing Lewis Structures** - Construct the Lewis structure for the molecule or ion based on the determined valence electrons. (c) **Resonance Hybrid Analysis** - Check if the molecule exists as a resonance hybrid. - If resonance exists, draw the resonance structures. - If not, indicate with "NA" for not applicable. (d) **Identifying Molecular Geometry** - Determine and state the name of the molecular geometry for the given molecule or ion. (e) **VSEPR Representation** - Draw the VSEPR (Valence Shell Electron Pair Repulsion) model of the molecular geometry using wedges and dashed lines as needed. Ensure to include the bond angles in your representation to provide a clear depiction of the molecular shape. **Exercise on Lewis Theory**1. **Problem 1: Aluminum Chloride Formation** - *Task:* Using Lewis theory, show how the formula for aluminum chloride is obtained.2. **Problem 2: Formation of an Ionic Compound** - *Task:* A metal \( M \) has two valence electrons and a non-metal \( N \) has five valence electrons. Using Lewis theory, predict the formula for this ionic compound. - *Note:* Instructor Initials __________3. **Problem 3: Chlorine Gas as a Diatomic Molecule** - *Task:* Using Lewis theory, show and explain why chlorine gas exists as a diatomic molecule.

The objective of the question is to explain the existence of nitrogen molecule as a diatomic…

4. Using Lewis theory, show and explain why nitrogen gas exists as a diatomic molecule. 5. For each molecule or ion complete the following: (a) Determine the total number of valence electrons available for bonding / electron-pairs available for bonding. (b) Draw the Lewis structure. (c) Determine whether the molecule exists as a resonance hybrid If it does, draw the resonance structures. If it does not, write "NA" for not applicable. ● ● (d) State the name of the molecular geometry (e) Draw the VSEPR representation of the molecular geometry using wedges and dashed lines where appropriate Include the bond angles. ●

4. Using Lewis theory, show and explain why nitrogen gas exists as a diatomic molecule. 5. For each molecule or ion complete the following: (a) Determine the total number of valence electrons available for bonding / electron-pairs available for bonding. (b) Draw the Lewis structure. (c) Determine whether the molecule exists as a resonance hybrid If it does, draw the resonance structures. If it does not, write "NA" for not applicable. ● ● (d) State the name of the molecular geometry (e) Draw the VSEPR representation of the molecular geometry using wedges and dashed lines where appropriate Include the bond angles. ●

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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