Chapter 14, Problem 3A

Interpretation Introduction

Interpretation: The atoms in addition to hydrogen which are necessary for hydrogen bonding needs to be explained. The contribution of small size of hydrogen atom to the unusual strength of dipole-dipole forces involved in hydrogen bonding needs to be explained.

Concept introduction: The hydrogen bond may be defined as strong dipole-dipole forces of attraction that operates between a hydrogen atom that is covalently bonded to an atom of high electronegativity.

Answer to Problem 3A

Fluorine, oxygen, and nitrogen in addition to hydrogen is needed for hydrogen bonding.

Explanation of Solution

The covalent bond between hydrogen and an electronegative element is considerably polar because the electronegative atom attracts the bonding electron towards itself. The partial positive charge on hydrogen attracts the partial negative charge of an electronegative atom forming what is called hydrogen bonding.

Due the very small size of the hydrogen atom the dipoles can approach each other closely which increases the strength of hydrogen bonding. Atoms bigger in size can disrupt the hydrogen bonding because it will find difficulty in coming closer to each other.

Conclusion

Fluorine, oxygen, and nitrogen in addition to hydrogen needed for hydrogen bonding.