Question

the imfs you selected are shown below, along with the molecular weights for the substances. based on those things, which substance below would you expect to have the higher boiling point? substance imfs molecular weight br-br london dispersion 160.0 g/mol cl-cl london dispersion 71.0 g/mol

Explanation:

Step1: Analyze the relationship between molecular weight and boiling point

Generally, for substances with the same type of intermolecular forces (IMFs), the higher the molecular weight, the stronger the London dispersion forces. Stronger intermolecular forces require more energy to break, so a higher boiling point is expected.

Step2: Compare the molecular weights of the two substances

The molecular weight of \(Br - Br\) is \(160.0\ g/mol\) and that of \(Cl - Cl\) is \(71.0\ g/mol\). Since \(160.0>71.0\) and both have London dispersion forces (the same type of IMF).

Answer:

\(Br - Br\)