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The electronegativity difference between \( \mathrm{N} \) and \( \mathrm{F} \) is greater than \( \mathrm{N} \) and \( \mathrm{H} \), yet the dipole moment of \( \mathrm{NH}_{3} \) \( (1.5 \mathrm{D}) \) is greater than that of \( \mathrm{NF}_{3}(0.2 \mathrm{D}) \). This is because:
(a) In \( \mathrm{NH}_{3} \) as well as \( \mathrm{NF}_{3} \), the atomic dipole and bond dipole are in the opposite direction
(b) In \( \mathrm{NH}_{3} \), the atomic dipole and bond dipole are in the opposite direction, 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 direction
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