Question

Which of the following compounds has the highest boiling point?

• A. \( \text{CH}_4 \)
• B. \( \text{H}_2O \)
• C. \( \text{NH}_3 \)
• D. \( \text{CO}_2 \)

Hint:

Hydrogen bonding significantly increases boiling points. Water's high boiling point is due to the strong hydrogen bonds between molecules.

Answer 1

The Correct Option is B

Boiling point depends on the strength of intermolecular forces. The stronger the intermolecular forces, the higher the boiling point. - \( \text{CH}_4 \) (methane) is a non-polar molecule with weak London dispersion forces, so it has a low boiling point. - \( \text{H}_2O \) (water) has hydrogen bonding, a strong intermolecular force, giving it a relatively high boiling point. - \( \text{NH}_3 \) (ammonia) also has hydrogen bonding, but it is weaker than that in water, so its boiling point is lower. - \( \text{CO}_2 \) (carbon dioxide) is a non-polar molecule with weak London dispersion forces, resulting in a low boiling point. Thus, \( \text{H}_2O \) has the highest boiling point due to its strong hydrogen bonding.