Of the two compounds in Question 23.10, which has the higher boiling point? Explain.

Name: Problem 11, Chapter 23: Chemistry The Molecular Nature of Matter
Uploaded: 2021-10-06T18:57:01-08:00
Duration: 4 min 4 s
Channel: Nicholas Sacco
Description: Of the two compounds in Question 23.10, which has the higher boiling point? Explain.

Of the two compounds in Question 23.10, which has the higher...

Key Concepts

Boiling Point

Boiling point is the temperature at which a liquid turns into a gas and is determined largely by the strength of the intermolecular forces present. In general, the stronger these forces, the higher the boiling point will be because more energy is needed to separate the molecules.

Intermolecular Forces

Intermolecular forces are the attractions between molecules that dictate many physical properties, including boiling point. They include various types, such as London dispersion forces, dipole-dipole interactions, and hydrogen bonding, each contributing differently to the overall intermolecular attraction.

Hydrogen Bonding

Hydrogen bonding is a particularly strong type of dipole-dipole interaction that occurs when hydrogen is bonded to highly electronegative atoms such as oxygen, nitrogen, or fluorine. Its presence in a compound significantly increases the boiling point because it leads to strong attractions between molecules.

London Dispersion Forces

London dispersion forces are weak intermolecular attractions that arise from temporary fluctuations in electron density in molecules. While they are generally the weakest type of intermolecular force, they become more significant in larger, non-polar molecules and can affect the boiling point.

Transcript

00:01 Okay, so examining the compounds in problem 10, we want to determine which one has the higher boiling point.

00:07 And there's a few trends that affect the boiling point.

00:15 And the first one is likely of the chain.

00:19 I mean, the type of bonding.

00:26 And the most important type of bonding, which is going to lead to the highest boiling point, is going to be ionic.

00:35 And then this is followed by hydrogen bonding, which is followed by diple -diple interactions or a pole.

00:47 Or cavil and bond and the last one is london dispersion forces or ldf so if a compound has a diple dipole interaction it's going to be more it's give a higher boiling point than one with just london dispersion forces and if it has hydrogen bonding it's going to be have a higher boiling point than just one like pull polar covalidem bonding the second point is the length of the chain so increasing the length of the chain is going to decrease the boiling point.

01:33 So if a smaller chain is going to have a higher boiling point than a larger one.

01:41 And the third point is branching.

01:44 And if this does occur, it's going to allow the boiling point as well.

01:47 Because we have less interaction between neighboring atoms.

01:52 And this is similar to the length of the chain.

01:54 So we have less, we have less surface area.

02:00 Oh, wait, wait, wait...