The dipole moment mu of CH_4 and CCl_4 is 0. | vedclass

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(C) Both $CH_4$ and $CCl_4$ have a dipole moment $\mu = 0$,which indicates that they are non-polar molecules.In these molecules,the central atom $(C)$

Vedclass · Accepted Answer

Tetrahedral

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(C) Both $CH_4$ and $CCl_4$ have a dipole moment $\mu = 0$,which indicates that they are non-polar molecules.In these molecules,the central atom $(C)$ is $sp^3$ hybridized.The four bonds are arranged symmetrically in space to minimize electron-pair repulsion.This arrangement results in a tetrahedral geometry with a bond angle of $109^{\circ} 28^{\prime}$.Because of this high symmetry,the individual bond dipoles cancel each other out,resulting in a net dipole moment of zero.

Molecule	$P-X$ (axial) bond length / $P-X$ (equatorial) bond length
$PF_5$	$a / b$
$PF_4CH_3$	$c / d$
$PF_3(CH_3)_2$	$e / f$
$PCl_5$	$g / h$

The dipole moment $\mu$ of $CH_4$ and $CCl_4$ is $0$. Predict their shapes. Provide the correct shape with reasons.

Similar Questions

The compound$(s)$ with $2$ lone pairs of electrons on the central atom is(are):
$(A)$ $BrF_5$
$(B)$ $ClF_3$
$(C)$ $XeF_4$
$(D)$ $SF_4$

Which of the following is the correct order of increasing number of lone pair of electrons on the central atom?

The shape of the $O_2F_2$ molecule is similar to which of the following?

Which of the following shapes is not possible for any possible value of $n$ in the $XeF_n$ molecule?

Consider the following information $(X = F$ or $Cl)$:

Molecule $P-X$ (axial) bond length / $P-X$ (equatorial) bond length

$PF_5$ $a / b$

$PF_4CH_3$ $c / d$

$PF_3(CH_3)_2$ $e / f$

$PCl_5$ $g / h$

According to the given information,choose the incorrect order of bond lengths.

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