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(A) The dipole moment depends on the electronegativity difference between the central atom and the surrounding atoms,as well as the molecular geometry

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$NH_3$

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(A) The dipole moment depends on the electronegativity difference between the central atom and the surrounding atoms,as well as the molecular geometry. In $NH_3$,the electronegativity difference between $N$ and $H$ is significant. The dipole moments of the three $N-H$ bonds and the lone pair on $N$ all point in the same direction,resulting in a large net dipole moment $(1.47 \ D)$. In $NCl_3$,the electronegativity of $N$ $(3.04)$ and $Cl$ $(3.16)$ are very similar. The dipole moments of the three $N-Cl$ bonds point in the opposite direction to the lone pair,leading to a smaller net dipole moment $(0.6 \ D)$. $CS_2$ has a linear geometry $(S=C=S)$,making it a non-polar molecule with a net dipole moment of $0 \ D$. $C_2H_6$ (ethane) is a non-polar hydrocarbon with a net dipole moment of $0 \ D$. Therefore,$NH_3$ has the maximum dipole moment among the given options.

Which of the following molecules has the maximum dipole moment?

Similar Questions

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