MHT CET Chemistry Question (2026) — Solution

Step-by-step solution

The dipole moment of a molecule depends on its geometry and the electronegativity difference between its constituent atoms. For H _2 O , the oxygen atom is highly electronegative and possesses two lone pairs. The molecule has a bent structure, and the bond dipoles along with the lone pair dipoles reinforce each other, resulting in a high dipole moment of approximately 1.85 D . For NH _3, the nitrogen atom has one lone pair and the molecule is trigonal pyramidal. Its dipole moment is approximately 1.47 D . For CHCl _3, the molecule has a tetrahedral geometry but is asymmetric. Its dipole moment is approximately 1.04 D . For BeF _2, the molecule is linear and symmetric. The two Be-F bond dipoles are equal and opposite, cancelling each other out and resulting in a dipole moment of 0 D . Thus, H _2 O has the highest dipole moment among the given molecules. Answer: H _2 O