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 :

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 . 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:

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:

The boiling points of hydrides of group 16 elements are in the order :

The boiling point of hydrides of group 16 elements are in the order.