Assign the oxidation state for nitrogen in each of the following. a \(\mathrm{L}_{3} \mathrm{N} \quad\) d. NO \(\quad\) g. \(\mathrm{NO}_{2}^{-}\) b. \(\mathrm{NH}_{3} \quad\) e. \(\mathrm{N}_{2} \mathrm{O} \quad\) h. \(\mathrm{NO}_{3}^{-}\) c\(\mathrm{N}_{2} \mathrm{H}_{4} \quad\) f. \(\mathrm{NO}_{2} \quad\) i. \(\mathrm{N}_{2}\)

In order to determine the oxidation states for nitrogen in each of the given compounds, we need to keep certain rules in mind: 1. The oxidation state of an element in its free elemental form is 0. 2. The oxidation state of a monoatomic Ion is equal to the charge it carries. 3. In a neutral compound, the sum of oxidation states is 0; in a polyatomic ion, the sum is equal to the charge of the ion. 4. The more electronegative element carries the negative oxidation state, and the less electronegative element carries the positive one.

a. Li3N - Lithium nitride Let's determine the oxidation state for N in Li3N. Li: +1 (alkali metals have +1 oxidation state) For three lithium atoms, the total charge is +3. To maintain neutrality in the compound, the nitrogen atom must carry a -3 charge. Oxidation state of N: -3 b. NH3 - Ammonia Let's determine the oxidation state for N in NH3. H: +1 For three hydrogen atoms, the total charge is +3. To maintain neutrality in the compound, the nitrogen atom must carry a -3 charge. Oxidation state of N: -3 c. N2H4 - Hydrazine Let's determine the oxidation state for N in N2H4. H: +1 For four hydrogen atoms, the total charge is +4. In order to maintain neutrality, the sum of the oxidation states of the two nitrogen atoms must be -4. Therefore, each nitrogen atom must carry an oxidation state of -2. Oxidation state of N: -2 d. NO - Nitrogen monoxide Let's determine the oxidation state for N in NO. O: -2 To maintain neutrality in the compound, the nitrogen atom must carry a +2 charge. Oxidation state of N: +2 e. N2O - Nitrous oxide Let's determine the oxidation state for N in N2O. O: -2 In order to maintain neutrality, the sum of the oxidation states of the two nitrogen atoms must be +2. Therefore, each nitrogen atom must carry an oxidation state of +1. Oxidation state of N: +1 f. NO2 - Nitrogen dioxide Let's determine the oxidation state for N in NO2. O: -2 For two oxygen atoms, the total charge is -4. To maintain neutrality in the compound, the nitrogen atom must carry a +4 charge. Oxidation state of N: +4 g. NO2- - Nitrite ion Let's determine the oxidation state for N in NO2-. O: -2 For two oxygen atoms, the total charge is -4. Since the charge of the ion is -1, the nitrogen atom must carry an oxidation state of +3. Oxidation state of N: +3 h. NO3- - Nitrate ion Let's determine the oxidation state for N in NO3-. O: -2 For three oxygen atoms, the total charge is -6. Since the charge of the ion is -1, the nitrogen atom must carry an oxidation state of +5. Oxidation state of N: +5 i. N2 - Nitrogen molecule Let's determine the oxidation state for N in N2. As N2 is an elemental form of nitrogen, the oxidation state for nitrogen is 0. Oxidation state of N: 0