The "O — N — O" bond angle is maximum in : — Chemical Bonding Chemistry Question

💡 Solution & Explanation

Step 1: Analyze the hybridization and electron geometry of each nitrogen species. Step 2: NO2^+ is a linear cation with sp hybridization and 0 lone pairs on the central nitrogen atom, giving a bond angle of 180°. NO2^- has sp2 hybridization with 1 lone pair, yielding a bent geometry with a bond angle of approximately 115°. NO3^- has sp2 hybridization with 0 lone pairs, giving a trigonal planar geometry with a 120° bond angle. Step 3: Since NO2^+ is linear, it possesses the maximum possible 'O-N-O' bond angle of 180°, matching option (b).