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  4. Arrange the following in order of increasing dipole moment: H2O, H2S, BF3

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Q. Arrange the following in order of increasing dipole moment: $H_{2}O, H_{2}S, BF_{3}$

Chemical Bonding and Molecular Structure

Solution:

In $BF_{3}$, dipole moment is zero due to its symmetrical structure. Summations of all dipoles is zero.
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In $H_{2}S$ and $H_{2}O$ due to unsymmetrical structure net $+$ ve dipole is there. $H_{2}O$ has higher dipole due to higher electronegativity of oxygen than sulphur.