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On the basis of intermolecular attractions, explain the differences in the boiling points of $n$ -butane $\left(-1^{\circ} \mathrm{C}\right)$ and chloreethane $\left(12^{\circ} \mathrm{C}\right),$ which have similar molar masses.
The boiling point of substances depends on the strength of intermolecular forces. More is the strength of intermolecular forces; more will be the boiling point and vice-versa.
01:17
Aadit S.
Chemistry 102
Chapter 10
Liquids and Solids
Liquids
Solids
University of Central Florida
Brown University
University of Toronto
Lectures
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So in this podcast we're going to be taking a look. Ah, boiling point And how this relates to into molecular forces. So, for example, with butane that's just a full carbon chain. This is non polar, so we have dispersion forces. However, due to the presence of CCL bonds, they we have dipole dipole interactions between Coral e thane. So what we have here is carbon carbon. We have a chlorine remainder of hydrogen ins. So here we have die Paul di poll contractions as well as dispassion forces. So due to the presence of the strong dipole dipole attractions, the boiling point of Clara within is greater than puting.
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