Question

22 ccc patterns explain whether hydrogen bonding is present between hydrogen fluoride (hf) molecules.

Explanation:

To determine hydrogen bonding in HF, recall the hydrogen bonding conditions: a hydrogen atom bonded to a highly electronegative atom (F, O, N) and a lone pair on a highly electronegative atom in another molecule. In HF, H is bonded to F (highly electronegative). The F atom in one HF molecule has lone pairs, and the H (with partial positive charge) from another HF molecule can be attracted to these lone pairs. So, hydrogen bonding occurs between HF molecules.

Answer:

Hydrogen bonding is present between hydrogen fluoride (HF) molecules. This is because in HF, hydrogen is bonded to fluorine (a highly electronegative atom). The fluorine atom in one HF molecule has lone pairs of electrons, and the partially positive - charged hydrogen atom of another HF molecule is attracted to the lone pairs on the fluorine atom of the first molecule, satisfying the conditions for hydrogen bonding (hydrogen bonded to F, O, or N and a lone pair on F, O, or N in a neighboring molecule).