**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 molecule.Nitrogen has five valence electrons. This suggests that it requires three electrons to complete its octet.The nitrogen gas molecule exists as a diatomic molecule (the two atoms are connected in a pair) where the nitrogen takes up three electrons from the other nitrogen atom to complete its octet.Determining the Lewis structure of nitrogen molecule -The total valence electrons in nitrogen molecule are calculated as follows-The nitrogen atom is bonded to another nitrogen atom by a triple bond suggesting the use of six valence electrons. The remaining four electrons appear as a lone pair of electrons on each nitrogen atom.The Lewis structure of the nitrogen atom is depicted as follows-Nitrogen has a small size and high electronegativity. It forms multiple bonds with itself as shown in Lewis structure. Thud, it exist as a diatomic molecule.Due to the small size and high electronegativity of a nitrogen atom, it forms multiple bonds with the other nitrogen atom and exists as a diatomic molecule.