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Chapter 11: Problem 48

Which would have the higher boiling point: chloroform, \(\mathrm{CHCl}_{3},\) or bromoform, \(\mathrm{CHBr}_{3}\) ?

Short Answer

Expert verified
Bromoform (CHBr3) would have a higher boiling point compared to Chloroform (CHCl3).

Step by step solution

01

Analyze the Molecular Weight

Bromoform uses Bromine, which has a molar mass of 79.9 g/mol, while Chloroform uses Chlorine, which has a molar mass of 35.5 g/mol. This means that Bromoform has a higher molecular weight.
02

Consider the Intermolecular Forces

Both Chloroform and Bromoform are polar molecules, which means they can form dipole-dipole interactions. However, because of the higher atomic radius and electron cloud of Bromine, Bromoform will have a higher capability of forming temporary dipoles, which will further strengthen its intermolecular forces.
03

Determine the Boiling Point

Considering that Bromoform, CHBr3, has both a higher molecular weight and stronger intermolecular forces (due to increased London dispersion forces), it will have a higher boiling point compared to Chloroform, CHCl3.

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