Step 1: Identify factors influencing boiling point
Boiling point is dictated by the strength of intermolecular forces. Greater intermolecular force strength correlates with higher boiling points.
Step 2: Evaluate and contrast the compounds
- \( \text{H}_2\text{O} \) (water) exhibits hydrogen bonding, a potent intermolecular force, resulting in an elevated boiling point.
- \( \text{CH}_4 \) (methane) possesses weak London dispersion forces, leading to a significantly low boiling point.
- \( \text{NH}_3 \) (ammonia) features hydrogen bonding, though its strength is less than that in \( \text{H}_2\text{O} \).
- \( \text{CO}_2 \) (carbon dioxide) is a nonpolar molecule characterized by weak dispersion forces, contributing to a low boiling point.
Step 3: Arrive at a conclusion
Given that water possesses the strongest hydrogen bonding, it will exhibit the highest boiling point among the provided substances.
Answer: Consequently, \( \text{H}_2\text{O} \) is the compound with the highest boiling point. Option (1) is therefore the correct selection.