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The electronegativity difference between \( \mathrm{N} \) and \( \mathrm{F} \) is greater than that between \( \mathrm{N} \) and \( \mathrm{H} \), yet the dipole moment of \( \mathrm{NH}_{3}(1.5 \mathrm{D}) \) is larger than that of \( \mathrm{NF}_{3}(0.2 \mathrm{D}) \). This is because:
(A) in \( \mathrm{NH}_{3} \) as well as in \( \mathrm{NF}_{3} \), the atomic dipole and bond dipole are in opposite directions
(B) in \( \mathrm{NH}_{3} \), the atomic dipole and bond dipole are in the opposite directions whereas in \( \mathrm{NF}_{3} \), these are in the same direction
(C) in \( \mathrm{NH}_{3} \) as well as in \( \mathrm{NF}_{3} \), the atomic dipole and bond dipole are in the same direction
(D) in \( \mathrm{NH}_{3} \), the atomic dipole and bond dipole are in the same direction whereas in \( \mathrm{NF}_{3} \), these are in the opposite directions
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