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
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
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