Dipole moment is a measure of the polarity of a molecule, which arises from the unequal sharing of electrons between atoms due to differences in electronegativity and the molecular geometry.

1. Dipole moment of H\u2082O:
Water ($H_{2}O$) has a bent structure due to two lone pairs on the oxygen atom. The O-H bonds are highly polar (oxygen is more electronegative than hydrogen). The bond dipoles add up constructively, resulting in a large net dipole moment. Dipole moment $\approx 1.85D$.

2. Dipole moment of NH\u2083:
Ammonia ($N{H}_3$) has a trigonal pyramidal structure with one lone pair on the nitrogen atom. The N-H bonds are polar (nitrogen is more electronegative than hydrogen). The bond dipoles and the lone pair dipole add up constructively, resulting in a significant net dipole moment. Dipole moment $\approx 1.47D$.

3. Dipole moment of NF\u2083:
Nitrogen trifluoride ($N{F}_3$) also has a trigonal pyramidal structure with one lone pair on the nitrogen atom. However, fluorine is more electronegative than nitrogen. The N-F bond dipoles point towards fluorine, away from the nitrogen atom. The lone pair dipole points away from the nitrogen atom. These bond dipoles largely cancel out the lone pair dipole, resulting in a very small net dipole moment. Dipole moment $\approx 0.23D$.

Comparing the values: $H_{2}O(1.85D)>N{H}_3(1.47D)>N{F}_3(0.23D)$.

Option Analysis:

• A) NF\u2083 > NH\u2083 > H\u2082O: Incorrect. NF\u2083 has the smallest dipole moment.
• B) NH\u2083 > NF\u2083 > H\u2082O: Incorrect. H\u2082O has the largest dipole moment.
• C) H\u2082O > NH\u2083 > NF\u2083: Correct. This order matches the calculated dipole moments.
• D) H\u2082O > NF\u2083 > NH\u2083: Incorrect. NH\u2083 has a larger dipole moment than NF\u2083.

Correct Answer: (C)