Both BF_3 and NH_3 are covalent molecules. Ho | vedclass

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

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$BF_3$ is planar while $NH_3$ is pyramidal.

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(D) $BF_3$ has a trigonal planar geometry with $sp^2$ hybridization. Due to its symmetric shape,the individual bond dipoles cancel each other out,resulting in a net dipole moment of $\mu = 0$. $NH_3$ has a trigonal pyramidal geometry with $sp^3$ hybridization,including one lone pair on the nitrogen atom. The lone pair and the three $N-H$ bonds do not cancel each other's dipole moments,resulting in a net dipole moment of $\mu 
eq 0$. Therefore,the difference in polarity arises from their molecular shapes: $BF_3$ is planar and $NH_3$ is pyramidal.

Both $BF_3$ and $NH_3$ are covalent molecules. However,$BF_3$ is non-polar while $NH_3$ is polar. What is the reason for this?

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Assertion $(A)$: Dipole moment of $NF_3$ is lesser than $NH_3$.
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The correct answer is:

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