Answer:
[tex]NH_3[/tex] > [tex]SbH_3[/tex] > [tex]AsH_3[/tex] > [tex]PH_3[/tex]
Explanation:
Boiling point increases with increase in intermolecular forces.
The two factors will be considered here for determining the trend for the boiling point of the hydrides of group 5A, which are:
Hydrogen bonding exists only in [tex]NH_3[/tex] as the difference in the electronegativity of the N and the H is large as compared to other elements of the group 5A.
The extent of the London forces increases with the increase in the molecular weight. Thus, [tex]SbH_3[/tex] must have the highest boiling point followed by [tex]AsH_3[/tex] , [tex]PH_3[/tex] and [tex]NH_3[/tex]. But hydrogen bonding is strongest intermolecular force. So the trend is:
[tex]NH_3[/tex] > [tex]SbH_3[/tex] > [tex]AsH_3[/tex] > [tex]PH_3[/tex]
Answer:
[tex]SbH_3>NH_3>AsH_3>PH_3[/tex]
Explanation:
Hello,
On the attached picture you will find a graph showing off the boiling point of the involved hydrides. In order to explain the exhibited behavior one must take into account that the higher the period of the group VA element's hydride, the higher the boiling point, nonetheless, ammonia shows an unexpected high boiling point which is possible due to the fact that nitrogen contains a small atomic number which is strongly electronegative with lone pairs, and which are strongly bonded to the hydrogen atoms. In spite of this, the tendency is conserved for phosphorous, arsenic and antimony since typical intermolecular interactions increase with increasing atomic number of the central atom in the molecule.
Best regards.
