${\rm{N}}{{\rm{H}}_3}$ has a net dipole moment, but boron trifluoride $\left( {{\rm{B}}{{\rm{F}}_3}} \right)$ has zero dipole moment, because:

${\rm{N}}{{\rm{H}}_3}$ is pyramidal while ${\rm{B}}{{\rm{F}}_3}$ is trigonal planar

$B$ is less electronegative than $N$

$F$ is more electronegative than $H$

${\rm{B}}{{\rm{F}}_3}$ is pyramidal while ${\rm{N}}{{\rm{H}}_3}$ is planar

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NEET UG CHEMISTRY MCQ: CHEMICAL BONDING & MOLECULAR STRUCTURE

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\mathrm{N}{\mathrm{H}_3}

has a net dipole moment, but boron trifluoride

\left( {\mathrm{B}{\mathrm{F}_3}} \right)

has zero dipole moment, because:

View answer and explanation

Correct option: D

\mathrm{N}{\mathrm{H}_3}

is pyramidal while

\mathrm{B}{\mathrm{F}_3}

is trigonal planar

Option D (

\mathrm{N}{\mathrm{H}_3}

is pyramidal while

\mathrm{B}{\mathrm{F}_3}

is trigonal planar) is correct because the geometry of the molecules determines whether the individual bond dipoles cancel out or add up to a net dipole moment.

NEET UG CHEMISTRY MCQ: CHEMICAL BONDING & MOLECULAR STRUCTURE

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