Which of the following statements regarding N | vedclass

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(C) Both $NH_3$ and $NF_3$ have a pyramidal geometry due to the presence of one lone pair on the central nitrogen atom and $sp^3$ hybridization.In $NH

Vedclass · Accepted Answer

The resultant dipole moment of $NH_3$ is $4.90 	imes 10^{-30} \ C \ m$ and that of $NF_3$ is $0.80 	imes 10^{-30} \ C \ m$.

Vedclass · Answer

(C) Both $NH_3$ and $NF_3$ have a pyramidal geometry due to the presence of one lone pair on the central nitrogen atom and $sp^3$ hybridization.In $NH_3$,the electronegativity of $N$ $(3.0)$ is greater than $H$ $(2.1)$,so the bond dipoles point towards $N$. The lone pair dipole also points in the same direction,leading to a large resultant dipole moment of $4.90 	imes 10^{-30} \ C \ m$.In $NF_3$,the electronegativity of $F$ $(4.0)$ is greater than $N$ $(3.0)$,so the bond dipoles point away from $N$. The lone pair dipole points towards $N$. These oppose each other,resulting in a smaller net dipole moment of $0.80 	imes 10^{-30} \ C \ m$.Therefore,statement $C$ is correct.

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 statements regarding $NH_3$ and $NF_3$ is correct?

Similar Questions

Which among the following molecules is non-polar?

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

Which bond is expected to be the least polar?

The order of dipole moments of the following molecules is

Consider the following:
Assertion $(A)$: Dipole moment of $NF_3$ is lesser than $NH_3$.
Reason $(R)$: In $NF_3$,the orbital dipole due to lone pair of electrons is in the opposite direction to the resultant dipole moment of the three $N-F$ bonds.
The correct answer is:

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