Import Question JSON

$\text{HINT: Molecule dipole moment is zero for symmetrical molecule.} \text{Explanation:} \text{1. } \text{CO}_2 \text{ is a symmetrical linear molecule, so the dipole moment is zero.} \text{2. In } \text{CH}_4 \text{, which is a tetrahedral molecule, the individual bond dipoles cancel each other out due to its symmetrical structure, resulting in a net dipole moment of zero.} \text{3. For } \text{NH}_3 \text{ (Ammonia), it has a trigonal pyramidal shape with a lone pair on the nitrogen atom. The bond dipoles of the N-H bonds and the lone pair moment add up in the same direction, resulting in a significant net dipole moment (approximately 1.46 D).} \text{4. For } \text{NF}_3 \text{ (Nitrogen trifluoride), it also has a trigonal pyramidal shape and a lone pair on nitrogen. However, the direction of the N-F bond dipoles is opposite to that of the lone pair moment on the nitrogen atom. This leads to a partial cancellation of dipoles, resulting in a much smaller net dipole moment (approximately 0.24 D) compared to } \text{NH}_3\text{.} \text{Comparing the dipole moments:} \text{CO}_2 \text{ (0 D)} \text{CH}_4 \text{ (0 D)} \text{NF}_3 \text{ (}\approx\text{0.24 D)} \text{NH}_3 \text{ (}\approx\text{1.46 D)} \text{Therefore, } \text{NH}_3 \text{ has the maximum dipole moment.}$