It is seen that there is a regular increase in boiling points of the hydrides of group 15 from P to Bi? Then why the hydride of nitrogen has higher boiling point than the hydride of phosphorous?

Asked by joykphukan | 16th Dec, 2015, 07:25: PM

Expert Answer:

In NH3, the molecules are associated by hydrogen bonding and thus its boiling point is comparatively high in comparison to PH3 and AsH3 which have no hydrogen bonding present.

On moving from PH3 to AsH3, boiling points increase due to increase in the magnitude of van der Waal’s forces due to increase in molecular size.

Hydride

NH3

PH3

AsH3

SbH3

BiH3

Boiling point(°C)

-33

-89

-63

-9

17

 

Answered by Vaibhav Chavan | 18th Dec, 2015, 12:30: PM

Queries asked on Sunday & after 7pm from Monday to Saturday will be answered after 12pm the next working day.