**Task: Draw the Lewis Structures for the Nitrate Ion (\(NO_3^-\))****Objective:** Illustrate three resonance forms for the nitrate ion. Ensure to include electron lone pairs and any formal charges in your diagrams.**Explanation:**1. **Understanding Resonance**: - Resonance in chemistry refers to the phenomenon where a molecule can be depicted using two or more structures, with electrons distributed differently between them. 2. **Structure Breakdown**: - **Nitrate Ion (\(NO_3^-\))**: This polyatomic ion consists of one nitrogen atom (N) bonded to three oxygen atoms (O). - The negative charge is distributed over the oxygen atoms.3. **Steps to Draw Lewis Structures**: - **Identify the total number of valence electrons**: Nitrogen contributes 5, each oxygen contributes 6, and the extra negative charge adds 1 more electron, totaling 24 valence electrons. - **Construct the basic skeletal structure**: Connect the nitrogen atom to each oxygen. - **Distribute the valence electrons**: Satisfy the octet rule for oxygen atoms. - **Assign formal charges**: Calculate the formal charge on each atom for each resonance structure to ensure the overall charge is -1.4. **Resonance Forms**: - The three resonance forms involve shifting the double bond between the nitrogen atom and each of the three oxygen atoms in turn. Each resonance form shows one double bond and two single bonds. 5. **Illustration Details**: - **Electron Lone Pairs**: Non-bonding electron pairs should be shown for the oxygen atoms. - **Formal Charges**: - The nitrogen atom typically has a formal charge of +1. - One of the oxygen atoms will have a -1 charge in each resonance form. - The remaining atoms should have formal charges of 0.Remember to depict these structures with clear bonds, correctly placed electron lone pairs, and formal charges for an accurate representation.

Lewis structure represents the systematic arrangement of atoms around the central atom. Electrons in this structure are indicated by dots. The central atom is the least electronegative element in a molecule. The given molecule is NO3−. Nitrogen (N) is more electronegative than oxygen (O). Therefore, N is the central atom in the molecule. The N atom has 5 valence electrons and O has 6 valence electrons. Calculate the total number of valence electrons in NO3−.Total number of valence electrons=5+3×6+1=24 The total number of valence electrons in NO3− is 24. The number of valence electron pairs is half of the total number of valence electrons. Therefore, the number of valence electron pairs in NO3− is 12, which is 24/2. Draw the skeletal structure of NO3− by assigning 3 valence electron pairs between N and O atoms (two on each side of N).The remaining valence electron pairs are assigned as the lone pairs to the surrounding three O atoms. In this way, 6 electron pairs are used. With the distribution of electron pairs the octet of oxygen is completed. The central N atom does not have a complete octet of electrons. Therefore, one electron each of N and O atom form two double bonds to complete the octet of N atom. Draw the complete Lewis dot structures and formal charges of NO3−.