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.

Explanation:

The hydrides of group 5A show an increase in boiling point from to . But boiling point of 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, will undergo strong hydrogen bonding.

In order to break this N-H bond, high temperature is required. Thus, boiling point of 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   to .

Whereas the boiling point of  is higher than those of and but lower than and because higher Vander waals forces of attraction more than compensates the increase in boiling point of because of hydrogen bonding.

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

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b. atoms in metallic solids are not arranged in a regular pattern

explanation: