8. Given the following species of nitrogen:oxygen containing molecules -NO^+,NO^2-,NO^3-which N-O bond is the strongest? __ The weakest? __

To determine which N-O bond is the strongest and which is the weakest among the given species \( NO^+ \), \( NO_2^- \), and \( NO_3^- \), we need to analyze the bond order of the N-O bonds in each molecule. Bond order is directly related to bond strength: higher bond order corresponds to a stronger bond, while lower bond order corresponds to a weaker bond.<br /><br />---<br /><br />### Step 1: Calculate the bond order for each species<br /><br />#### (a) \( NO^+ \):<br />- The Lewis structure of \( NO^+ \) shows a triple bond between nitrogen and oxygen.<br />- Bond order = 3.<br /><br />#### (b) \( NO_2^- \):<br />- The Lewis structure of \( NO_2^- \) has resonance structures, where the two N-O bonds are equivalent due to delocalization of electrons.<br />- Bond order = \( \frac{1 + 1 + 2}{2} = 1.5 \).<br /><br />#### (c) \( NO_3^- \):<br />- The Lewis structure of \( NO_3^- \) also has resonance structures, where the three N-O bonds are equivalent due to delocalization of electrons.<br />- Bond order = \( \frac{1 + 1 + 1}{3} = 1.33 \).<br /><br />---<br /><br />### Step 2: Compare bond orders<br />- \( NO^+ \): Bond order = 3 (strongest bond).<br />- \( NO_2^- \): Bond order = 1.5.<br />- \( NO_3^- \): Bond order = 1.33 (weakest bond).<br /><br />---<br /><br />### Final Answer:<br />- **Strongest N-O bond**: \( NO^+ \) (bond order = 3).<br />- **Weakest N-O bond**: \( NO_3^- \) (bond order = 1.33).