Which of the following is not a best representation of the H-bond? — Chemical Bonding Chemistry Question

💡 Solution & Explanation

Step 1: For a molecule to possess a permanent dipole moment (μ ≠ 0), it must have an asymmetrical geometry so that the individual bond dipoles do not cancel out. Step 2: Evaluate the options: CO_2 (linear, μ = 0) and SiF_4 (regular tetrahedral, μ = 0) are symmetrical and non-polar. NO_2 is a bent molecule (μ ≠ 0), and O_3 is also bent with a lone pair on the central oxygen (μ ≠ 0). Step 3: Since both NO_2 and O_3 are bent and asymmetrical, they both possess permanent dipole moments. Thus, the correct option is (b).