Draw a Lewis dot diagram for \(\mathrm{NO}_{3}^{-}\), and use the oxidation- state method of electron bookkeeping to determine how many electrons each atom should be assigned.

To draw the Lewis dot diagram of the NO₃⁻ ion, follow these steps: a. Determine the number of valence electrons for each atom and ion charge. b. Arrange the atoms with the central atom (N) in the middle surrounded by oxygen atoms. c. Complete the octets for the surrounding atoms (O) by adding lone pairs and forming bonds with the central atom (N). a. Number of valence electrons: Nitrogen (N): 5 valence electrons. Oxygen (O) - has 3 atoms: 6 × 3 = 18 valence electrons. Overall charge of the ion (-1): 1 valence electron. Total valence electrons: 5 + 18 + 1 = 24 valence electrons. b. Atom arrangement: O-N-O, with the 3rd oxygen on top or below the nitrogen atom. c. Complete octets: 1. Connect each O atom to the N atom with a single bond; each bond consumes 2 electrons. Now, we've used 6 out of 24 electrons. 2. Place lone pairs on each oxygen atom to complete their octets; each O needs 6 more electrons. We have (24 - 6) = 18 electrons left, which are enough to complete the octets. 3. Add a double bond between one O and N to satisfy N atom's octet rule. Now, all atoms have complete octets, and we've used all 24 valence electrons. The Lewis dot structure for NO₃⁻ ion will be: O⁻-N=O | O⁻

To determine the oxidation state of each atom in the NO₃⁻ ion, follow these rules: 1. The sum of oxidation states for all atoms in a compound is equal to the overall charge (in our case, it's -1). 2. Oxygen's oxidation state is usually -2. 3. Nitrogen's oxidation state is variable but will be determined based on the total oxidation state of the ion. Applying these rules: Oxygen - has 3 atoms, and each atom has an oxidation state of -2, so the total charge = -2 × 3 = -6. Now add +x for Nitrogen, where x is the oxidation state of Nitrogen. The sum of oxidation states equation will be: x - 6 = -1.

To find the nitrogen oxidation state and assigned electrons for each atom, solve the equation from step 2. Equation: x - 6 = -1 ➡ x = -1 + 6 ➡ x = 5 So, the oxidation state of nitrogen is +5. Finally, we can determine the number of assigned electrons for each atom: 1. Nitrogen (N): The assigned electrons = [# of valence electrons] - [oxidation state] = 5 - 5 = 0 2. Oxygen (O) - each atom: The assigned electrons = [# of valence electrons] - [oxidation state] = 6 - (-2) = 6 + 2 = 8 In the NO₃⁻ ion, each oxygen atom is assigned 8 electrons, while nitrogen is assigned 0 electrons using the oxidation-state method.