Rank from highest to lowest melting point

Asked by maham237 @ 03/01/2021 in Chemistry viewed by 294 People

The hydrides of group 5A are NH3, PH3, AsH3, and SbH3. Arrange them from highest to lowest boiling point.
Rank the molecules from highest to lowest boiling point. To rank items as equivalent, overlap them.

Answered by maham237 @ 03/01/2021

Explanation:

The hydrides of group 5A show an increase in boiling point from $PH_{3}$ to $BiH_{3}$ . But boiling point of $NH_{3}$ is higher than rest of the hydrides of group 5A.

This is because electronegativity of nitrogen is higher than hydrogen. So, it will attract electrons of hydrogen more towards itself. Thus, polarity will develop between nitrogen and hydrogen bond. As a result, $NH_{3}$ will undergo strong hydrogen bonding.

In order to break this N-H bond, high temperature is required. Thus, boiling point of $NH_{3}$ will be high.

On the other hand, on moving down the group there will be an increase in mass. Thus, there will be increase in Vander waals forces of attraction and as a result, there will be increase in boiling point from $PH_{3}$ to $BiH_{3}$ .

Whereas the boiling point of $NH_{3}$ is higher than those of $PH_{3}$ and $AsH_{3}$ but lower than $SbH_{3}$ and $BiH_{3}$ because higher Vander waals forces of attraction more than compensates the increase in boiling point of $NH_{3}$ because of hydrogen bonding.

Thus, the order from highest to lowest boiling point for hydrides of group 5A are as follows.

$BiH_{3}$ > $SbH_{3}$ > $NH_{3}$ > $AsH_{3}$ > $PH_{3}$

Rank from highest to lowest melting point

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