Which molecule does not show zero dipole mome | vedclass

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(B) The dipole moment of a molecule is zero if it has a symmetrical geometry where the bond dipoles cancel each other out. $BF_3$ is trigonal planar,$

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$NH_3$

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(B) The dipole moment of a molecule is zero if it has a symmetrical geometry where the bond dipoles cancel each other out. $BF_3$ is trigonal planar,$CCl_4$ is tetrahedral,and $CH_4$ is tetrahedral; all these have a net dipole moment of $0 \ D$. $NH_3$ has a trigonal pyramidal geometry with a lone pair on the nitrogen atom,which results in a net dipole moment of approximately $1.47 \ D$. Therefore,$NH_3$ does not show zero dipole moment.

Which molecule does not show zero dipole moment?

Similar Questions

Assertion : Molecules of larger size have higher polarizability.
Reason : Polarizability is observed only in those molecules which have a permanent dipole moment.

The dipole moments of $CCl_{4}$,$CHCl_{3}$ and $CH_{4}$ are in the order:

Which of the following molecules has a zero dipole moment?

Dipole moment of $HCl = 1.03 \ D$ and $HI = 0.38 \ D$. Bond length of $HCl = 1.3 \ \mathring{A}$ and $HI = 1.6 \ \mathring{A}$. The ratio of the fraction of electric charge,$\delta$,existing on each atom in $HCl$ and $HI$ is:

Dipole moment of $HCl = 1.03 \ D$,$HI = 0.38 \ D$. Bond length of $HCl = 1.3 \ \mathring{A}$ and $HI = 1.6 \ \mathring{A}$. The ratio of the fraction of electric charge,$\delta$,existing on each atom in $HCl$ and $HI$ is

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