Identify the correct orders against the property mentioned: A. \ce{H2O} > \ce{NH3} > \ce{CHCl3} — dipole moment B. \ce{XeF4} > \ce{XeO3} > \ce{XeF2} — number of lone pairs on central atom C. \ce{O-H} > \ce{C-H} > \ce{N-O} — bond length D. \ce{N2} > \ce{O2} > \ce{H2} — bond enthalpy Choose the answer from the options given below:

Solution & Explanation

\textbf{Answer:} (C) A, D only \textbf{Solution:} A is correct: \ce{H2O} ($1.85\,\text{D}$) > \ce{NH3} ($1.47\,\text{D}$) > \ce{CHCl3} ($\sim 1.04\,\text{D}$). D is correct: bond enthalpy follows bond order/strength \ce{N2} (triple, $946$) > \ce{O2} (double, $498$) > \ce{H2} (single, $436$). B is wrong (\ce{XeF2} has 3 lone pairs > \ce{XeF4} has 2 > \ce{XeO3} has 1) and C is wrong. So A and D only.