BF_3 and NF_3 are both covalent compounds. Ho | vedclass

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(D) $BF_3$ has a trigonal planar geometry with $sp^2$ hybridization. Due to its symmetry,the individual bond dipole moments cancel each other out,resu

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$BF_3$ is planar,whereas $NF_3$ has a pyramidal shape

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(D) $BF_3$ has a trigonal planar geometry with $sp^2$ hybridization. Due to its symmetry,the individual bond dipole moments cancel each other out,resulting in a net dipole moment of $0$ (non-polar).$NF_3$ has a trigonal pyramidal geometry with $sp^3$ hybridization and one lone pair on the nitrogen atom. Due to the presence of the lone pair and the difference in electronegativity,the bond dipoles do not cancel out,resulting in a net dipole moment (polar).

List-$I$ (Molecules)	List-$II$ (Dipole moment)
$A$. $HBr$	$I$. $1.04$
$B$. $H_2S$	$II$. $0$
$C$. $NH_3$	$III$. $0.79$
$D$. $CHCl_3$	$IV$. $0.95$
	$V$. $1.47$

$BF_3$ and $NF_3$ are both covalent compounds. However,$BF_3$ is non-polar,while $NF_3$ is polar because .....

Similar Questions

Which of the following molecules has zero dipole moment?

Match the following molecules in List-$I$ with their respective dipole moments in List-$II$.
List-$I$ (Molecules) List-$II$ (Dipole moment)
$A$. $HBr$ $I$. $1.04$
$B$. $H_2S$ $II$. $0$
$C$. $NH_3$ $III$. $0.79$
$D$. $CHCl_3$ $IV$. $0.95$
$V$. $1.47$

The correct order of dipole moment is

The correct set of species with zero dipole moment is:
$(i) \, CO_2, \, (ii) \, COCl_2, \, (iii) \, CH_2Cl_2, \, (iv) \, BCl_3$

Which one of the following has the highest dipole moment?
$(i)$ $CH_2Cl_2$
$(ii)$ $CHCl_3$
$(iii)$ $CCl_4$

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