Which of the following molecules has the high | vedclass

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(B) The dipole moment depends on the molecular geometry and the electronegativity difference between the atoms. $BF_3$ has a trigonal planar geometry,

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$NH_3$

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(B) The dipole moment depends on the molecular geometry and the electronegativity difference between the atoms. $BF_3$ has a trigonal planar geometry,and the bond dipoles cancel each other out,resulting in a net dipole moment of $0 \ D$. In $NH_3$ and $NF_3$,both have a trigonal pyramidal geometry with a lone pair on the nitrogen atom. In $NH_3$,the direction of the bond dipoles $(N-H)$ and the lone pair dipole are in the same direction,reinforcing each other,leading to a high dipole moment of approximately $1.46 \ D$. In $NF_3$,the bond dipoles $(N-F)$ are in the opposite direction to the lone pair dipole,which partially cancels the net dipole moment,resulting in a lower value of approximately $0.24 \ D$. $B_2H_6$ (diborane) is a non-polar molecule with a bridged structure,resulting in a net dipole moment of $0 \ D$. Therefore,$NH_3$ has the highest dipole moment.

$1$. Burning candle	$i$. Line spectrum
$2$. Sodium vapour	$ii$. Continuous spectrum
$3$. Bunsen flame	$iii$. Band spectrum
$4$. Dark lines in solar spectrum	$iv$. Absorption spectrum

Which of the following molecules has the highest dipole moment?

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