Amongst BeF_{2},BF_{3},H_{2}O,NH_{3},CCl_{4} | vedclass

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Question

(A) The net dipole moment $(\mu_{net})$ depends on the molecular geometry and the electronegativity difference between atoms.
$BeF_{2}$ is linear,$BF

Vedclass · Accepted Answer

$3$

Vedclass · Answer

(A) The net dipole moment $(\mu_{net})$ depends on the molecular geometry and the electronegativity difference between atoms.
$BeF_{2}$ is linear,$BF_{3}$ is trigonal planar,and $CCl_{4}$ is tetrahedral. These molecules have symmetric structures where individual bond dipoles cancel each other out,resulting in $\mu_{net} = 0$.
$H_{2}O$ (bent),$NH_{3}$ (trigonal pyramidal),and $HCl$ (heteronuclear diatomic) have asymmetric charge distributions,resulting in $\mu_{net} 
eq 0$.
Therefore,the molecules with non-zero net dipole moment are $H_{2}O$,$NH_{3}$,and $HCl$.
The total count is $3$.

Amongst $BeF_{2}$,$BF_{3}$,$H_{2}O$,$NH_{3}$,$CCl_{4}$ and $HCl$,the number of molecules with non-zero net dipole moment is ...... .

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