SbH3 has more boiling point than NH3.
- In NH3, Hydrogen is bonded with hydrogen bonding. Hence the boiling point is comparatively lower due to weaker forces of attraction.
- As we go down the group of the periodic table, the size of an element increases, hence van der Waal's forces also increase as the element size increases.
- Higher force leads to higher boiling points, Since Nitrogen lies on the top of the 15th group it has a lesser boiling point than SbH3 as antimony lies below nitrogen in the 15th group.
- As we go down the group the stability of the hydrides decreases generally. Hence, the stability also decreases. Therefore the boiling points of hydrides increase as we go down the group.
- Considering the factors Hydrogen bonding, Metal size, Forces of attraction between each element and its hydride, we can conclude that the compund SbH3 boiling point is higher than NH3.
Therefore, SbH3 has a higher boiling point than NH3.
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Due to increase in size of central atom from N to Sb, the van der Waals forces increase. Therefore boiling point of SbH3 is more than that of NH3.
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Hydrogen bond in NH3 is capable of making the boinling point of NH3 higher than PH3 and AsH3. Since molecular mass of Sb>>N, the vanderwaal forces are comparatively more than intermolecular h-bonding
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thank you
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ok
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even though it has hydrogen bonding ...Hydrogen bonding with N is not that strong to overcome Molecular attractions in SbH3 ...due to size
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But NH3 has hydrogen bonding which is stronger than VWF
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