Question

chf₃ has a normal boiling point of -82.1°c, and chcl₃ has a normal boiling point of 61.2°c. which of the following best helps to explain why chcl₃ has a higher boiling point? a chcl₃ has dipole - dipole forces, but chf₃ does not. b chcl₃ experiences hydrogen bonding, but chf₃ does not. c chcl₃ has stronger london dispersion forces than chf₃ does. d chcl₃ has stronger covalent bonds than chf₃ does.

Explanation:

Boiling - point is related to intermolecular forces. Both \(CHF_3\) and \(CHCl_3\) have dipole - dipole forces. Neither has hydrogen bonding as hydrogen is not bonded to a highly electronegative atom like \(N\), \(O\), or \(F\) in a way to cause hydrogen bonding. Covalent bonds within the molecules do not directly affect boiling points which are about separating molecules from each other. London dispersion forces increase with molar mass. \(CHCl_3\) has a higher molar mass than \(CHF_3\), so it has stronger London dispersion forces which require more energy to overcome, resulting in a higher boiling point.

Answer:

C. \(CHCl_3\) has stronger London dispersion forces than \(CHF_3\) does.