Which of the following would have a permanent | vedclass

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Question

(C) The dipole moment of a molecule depends on its geometry and the polarity of its bonds.$BF_3$ has a trigonal planar geometry,$SiF_4$ has a tetrahed

Vedclass · Accepted Answer

$SF_4$

Vedclass · Answer

(C) The dipole moment of a molecule depends on its geometry and the polarity of its bonds.$BF_3$ has a trigonal planar geometry,$SiF_4$ has a tetrahedral geometry,and $XeF_4$ has a square planar geometry. Due to their high symmetry,the bond dipoles in these molecules cancel each other out,resulting in a net dipole moment of zero.$SF_4$ has a see-saw geometry due to the presence of one lone pair on the sulfur atom. This lack of symmetry prevents the bond dipoles from canceling out,resulting in a permanent dipole moment.

List-$I$ (Molecule)	List-$II$ (Dipole moment in $D$)
$A. HCl$	$I. 1.07$
$B. NH_3$	$II. 1.85$
$C. H_2O$	$III. 0.23$
$D. NF_3$	$IV. 1.47$

Which of the following would have a permanent dipole moment?

Similar Questions

Choose the correct option for the following molecule in view of chemical bonding:
$Cl-CH=C=C=CH-Cl$

Which of the following molecules is non-polar in nature?

Match the following:
List-$I$ (Molecule) List-$II$ (Dipole moment in $D$)
$A. HCl$ $I. 1.07$
$B. NH_3$ $II. 1.85$
$C. H_2O$ $III. 0.23$
$D. NF_3$ $IV. 1.47$
The correct answer is

Explain why $BeH_{2}$ molecule has a zero dipole moment although the $Be-H$ bonds are polar.

"Dipole moment is a vector quantity." What does this mean? How is it represented?

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