Question

Consider the substances hydrogen (H2), fluorine (F2), and hydrogen fluoride (HF). Based on their molecular structures, how does the boiling point of HF compare with the boiling points of H2 and F2?

The boiling point of HF is (higher than, lower than, similar to) the boiling point of H2, and it is (higher than, lower than, similar to) the boiling point of F2.

Answer 1

Both blanks are "higher than".

Step-by-step explanation:

Answer 2

The boiling point of HF is higher than the boiling point of H2, and it is higher than the boiling point of F2.

Step-by-step explanation:

In HF, inter- molecule forces will be present between the hydrogen and fluorine atoms. There will be hydrogen bonding present among the hydrogen and fluorine atoms. Hydrogen bonds are strong bonds and hence the boiling point for HF would be high as much energy will be required to break these bonds.

H2 and F2 will only have intra-molecular attractions and there will be no hydrogen bonds present in them. As a result, their boiling point will be lower.