Question

Which of the following compounds has the highest boiling point?

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

Hint:

Remember: Hydrogen bonding generally leads to higher boiling points compared to compounds with only dispersion forces.

Answer 1

The Correct Option is A

Step 1: Understand the factors affecting boiling point
The boiling point of a compound is determined by the strength of intermolecular forces: - Stronger intermolecular forces lead to higher boiling points.

Step 2: Compare the compounds
- \( \text{H}_2\text{O} \) (water) has hydrogen bonding, which is a strong intermolecular force, leading to a high boiling point.
- \( \text{CH}_4 \) (methane) has weak London dispersion forces, leading to a very low boiling point.
- \( \text{NH}_3 \) (ammonia) has hydrogen bonding, but it is not as strong as in \( \text{H}_2\text{O} \).
- \( \text{CO}_2 \) (carbon dioxide) is a nonpolar molecule with weak dispersion forces, leading to a low boiling point.
Step 3: Conclusion
Since water has the strongest hydrogen bonding, it will have the highest boiling point among the given options.
Answer: Therefore, the compound with the highest boiling point is \( \text{H}_2\text{O} \). So, the correct answer is option (1).