Which of the following has the highest boiling point? Hint: They are all nonpolar. \[ \mathrm{CH}_{4} \] \( \mathrm{CH}_{3} \mathrm{CH}_{3} \) \( \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3} \) \( \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3} \)

The highest boiling point among these nonpolar molecules belongs to \( \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3} \) (butane). This is due to its longer carbon chain, which increases the surface area and consequently, the van der Waals forces that hold the molecules together, requiring more energy (in the form of heat) to break apart those interactions during the phase transition. In practical terms, understanding boiling points is crucial for applications in fields like cooking and distillation. For example, in culinary practices, knowing that butane has a higher boiling point than methane can help when trying to achieve certain cooking techniques, such as frying or boiling, where maintaining specific temperatures is essential to the outcome of the dish.