The dipole moment of ${\rm{CHC}}{{\rm{l}}_3}$ is $1.05$ debye while that of ${\rm{CC}}{{\rm{l}}_4}$ is zero, because ${\rm{CC}}{{\rm{l}}_4}$ is:

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JEE CHEMISTRY MCQ: CHEMICAL BONDING & MOLECULAR STRUCTURE

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The dipole moment of

\mathrm{CHC}{\mathrm{l}_3}

1.05

debye while that of

\mathrm{CC}{\mathrm{l}_4}

is zero, because

\mathrm{CC}{\mathrm{l}_4}

is:

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Correct option: D

Regular tetrahedral

Option D (Regular tetrahedral) is correct because the symmetrical tetrahedral shape of CCl4 results in the cancellation of individual bond dipoles, leading to a zero net dipole moment.

JEE CHEMISTRY MCQ: CHEMICAL BONDING & MOLECULAR STRUCTURE

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