Answer:
The arrangement of the hydrides of group 5A from the highest to lowest boiling point is as follows:
SbH₃ > NH₃> AsH₃ > PH₃
Explanation:
The concept used in the question is molecular weight and intermolecular forces. The first step is to check intermolecular forces in the given hydrides. After that, the molecular weight is taken into account for ranking the molecules.
Further Explanation:
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.
Hence, the arrangement of the hydrides of group 5A from the highest to lowest boiling point is as follows:
SbH₃ > NH₃> AsH₃ > PH₃
Learn More:
boiling point of hydrides: brainly.com/question/11586812 ; Answered by: AsiaWoerner
Learn more :
about relationship between boiling point and intermolecular forces: brainly.com/question/3472771; Answered by: guesst555
Keyword:
Arrangement of the Hydrides of Group 5A, Electro-Negativity difference in the Molecules, NH₃ Molecule has more Electronegative Nitrogen and Hydrogen.