The correct order of dipole moment is :A CH4 < NF3 < NH3 < H2O B NF3 < CH4 < NH3 < H2O C NH3 < NF3 < CH4 < H2O D H2O < NH3 < NF3 < CH4

To determine the correct order of dipole moment, we need to consider the polarity of the molecules. The dipole moment is a measure of the separation of positive and negative charges within a molecule.

In general, molecules with polar bonds will have a higher dipole moment compared to molecules with nonpolar bonds. Additionally, the shape of the molecule also affects the dipole moment.

Let's analyze the given options:

A) CH4 < NF3 < NH3 < H2O B) NF3 < CH4 < NH3 < H2O C) NH3 < NF3 < CH4 < H2O D) H2O < NH3 < NF3 < CH4

Starting with option A, we have CH4, which is a tetrahedral molecule with four nonpolar C-H bonds. NF3 is a trigonal pyramidal molecule with three polar N-F bonds. NH3 is a trigonal pyramidal molecule with three polar N-H bonds. H2O is a bent molecule with two polar O-H bonds.

Comparing the dipole moments, we can see that H2O has the highest dipole moment due to its bent shape and polar O-H bonds. NH3 has the next highest dipole moment, followed by NF3. CH4, being a nonpolar molecule, has the lowest dipole moment.

Therefore, the correct order of dipole moment is:

D) H2O < NH3 < NF3 < CH4