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Fifth group elements form hydrides to ty...

Fifth group elements form hydrides to type `AH_(3)`. The hydrides have a lone pair of electrons. The hydries are reducing in nature and the reducing power is related to the stability of A-H bonds. The hydrides are covalent and low boiling. Their boiling points depends on their ability to from hydrogen bond and their molecular size which decide the intermolcular forces in the hydrides .
The boiling points of the hydrides of V-group elements are in the order :

A

`NH_(3) gt PH_(3) gt AsH_(3) gt Sbh_(3) `

B

`NH_(3) gt AsH_(3) gt SbH_(3) gtPH_(3)`

C

`SbH_(3) gt NH_(3) gt AsH_(3) gt PH_(3) `

D

`AsH_(3) gt SbH_(3) gt NH_(3) gt PH_(3) `

Text Solution

Verified by Experts

The correct Answer is:
C
Due to increase in size from `PH_(3)` to `SbH_(3)` the van der Waal's forces increase. So their boiling points increase from `PH_(3)` to `SbH_(3)` But due to intermolecular hydrogen bonding, `NH_(3)` has very high boiling point, but less than that of `SbH_(3)`.
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Fifth group elements form hydrides to type AH_(3) . The hydrides have a lone pair of electrons. The hydries are reducing in nature and the reducing power is related to the stability of A-H bonds. The hydrides are covalent and low boiling. Their boiling points depends on their ability to from hydrogen bond and their molecular size which decide the intermolcular forces in the hydrides . Reducing power of V-group hydrides are in order :

Fifth group elements form hydrides to type AH_(3) . The hydrides have a lone pair of electrons. The hydries are reducing in nature and the reducing power is related to the stability of A-H bonds. The hydrides are covalent and low boiling. Their boiling points depends on their ability to from hydrogen bond and their molecular size which decide the intermolcular forces in the hydrides . The H-M-H bond angle of V group hydrides decrease from 107^(circ) to 90^(circ) for NH_(3) to SbH_(3) , this is due to:

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