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The order given in my book is

$$\ce{NH3} > \ce{SbH3} > \ce{AsH3} > \ce{PH3}$$

Phosphorous is more electronegative than arsenic and antimony. Then shouldn't the dipole moment be more in case of $\ce{PH3}?$

And why does the anomaly of $\ce{NH3}$ occur?

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    $\begingroup$ Geometry/symmetry also has a role in determining the dipole, for example, if the molecules were planar as is $\ce{BF3}$ the dipole would be zero. $\endgroup$ – porphyrin Aug 16 at 16:56
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    $\begingroup$ @porphyrin could you convert this into a proper answer for this question $\endgroup$ – Stan Aug 16 at 17:59

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