The hydrides of group 5A are NH3, PH3, AsH3, and SbH3. Arrange them from highest to...

The hydrides of group 5A are NH3, PH3, AsH3, and SbH3. Arrange them from highest to lowest boiling point.

Expert Solution

Answer:-

The arrangement of the hydrides of group 5A from the highest to lowest boiling point is :-

SbH₃ > NH₃> AsH₃ > PH₃

The covalent bond is present in all the hydrides of Group 5A. Intermolecular forces and molecular weight affect the boiling point of these hydrides. Hydrogen bonding is formed because of high electro-negativity difference in the molecules and it is proportional to polarity.

Compounds with higher intermolecular force have higher boiling points. This is because, during the phase transition, they require more energy to able to break the bonds. Among the hydrides, NH₃ has hydrogen bond while SbH₃, AsH₃ and PH₃ are shown London-dispersion forces and dipole-dipole interactions.

Compared to PH₃ and AsH₃, SbH₃ has the highest boiling point due to its high molecular weight. After that, the boiling point of AsH₃ is higher than PH₃.

Compared to dipole-dipole and London-dispersion forces, the Hydrogen-bonding is strong. Therefore, the boiling point of NH₃ would be higher than the other three elements. But the molar mass of SbH₃ is greater than as compared to NH₃ and SbH₃ would have a higher London-dispersion force. Therefore, the boiling point of NH₃ is less as compared to SbH₃.

gladiator answered 2 years ago

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