Question

How do the strengths of London forces compare in \(\mathrm{CO}_{2}(l)\) and \(\mathrm{CS}_{2}(l) ?\) Which of these is expected to have the higher boiling point? How would you check your answer?

Short answer

CS2 is expected to have a higher boiling point than CO2 due to stronger London dispersion forces, as it has a larger molar mass and more polarizable electron cloud. Boiling points from reliable data sources can be used to confirm this.

Step-by-step solution

Understanding London Forces

London dispersion forces are weak intermolecular forces resulting from temporary dipoles that occur in molecules. These forces are present in all molecular substances and are stronger in molecules with larger molar masses and more diffuse electron clouds.

Compare Molar Masses

The strength of London forces generally increases with increasing molar mass of the molecule. Compare the molar masses of A liquid with stronger intermolecular forces will generally have a higher boiling point because more energy is required to overcome these forces and convert the liquid to a gas.

Analyze Electron Clouds

Besides molar mass, the shape and size of the electron clouds can also contribute to the strength of London forces. Larger or more polarizable electrons clouds will lead to stronger London dispersion forces.

Checking the Answer

To check the prediction, you can look up the boiling points of both CO2 and CS2. Alternatively, you may conduct an experiment to measure the boiling points of both liquids, but typically such information is available in chemical data references.

Key concepts

Intermolecular Forces

Intermolecular forces are the forces which mediate interaction between molecules, including attractions or repulsions. These forces dictate many of the physical properties of substances, such as boiling and melting points, viscosity, and surface tension. London dispersion forces, a type of intermolecular force, are particularly significant in nonpolar molecules.

Despite being the weakest type of intermolecular force, London dispersion forces are omnipresent in molecules. They arise due to momentary fluctuations in electron distribution within molecules, leading to the creation of temporary dipoles. These dipoles can induce other dipoles in neighboring molecules, thus causing an attraction between them. It's crucial to remember that London dispersion forces, while weak on their own, can have cumulative effects that influence a substance's physical properties.

Boiling Point Comparison

Boiling point is a fundamental physical property that can indicate the strength of intermolecular forces within a liquid. It’s the temperature at which the vapor pressure of a liquid equals the external pressure. Substances with stronger intermolecular forces require more energy—in the form of heat—to break these forces, leading to a higher boiling point.

A direct comparison of boiling points can reveal which substance has stronger intermolecular London dispersion forces. The substance with the higher boiling point is generally the one with stronger dispersion forces, as more heat is needed to overcome these attractions and allow molecules to enter the gas phase.

Molar Mass Effect on London Forces

Molar mass plays a significant role in the strength of London dispersion forces. The larger the molar mass, the more electrons a molecule has, which generally leads to a larger, more polarizable electron cloud.

As molar mass increases, the electron cloud becomes more susceptible to fluctuations, which enhance the molecule's ability to induce temporary dipoles in neighboring molecules. This results in stronger London dispersion forces. Consequently, comparing the molar masses of two substances helps predict which will have the larger dispersion forces and, often, the higher boiling point. In the context of \( \mathrm{CO}_{2}(l) \) and \( \mathrm{CS}_{2}(l) \), \( \mathrm{CS}_{2} \) with a higher molar mass is predicted to exhibit stronger London forces and a higher boiling point.

Electron Cloud Polarizability

Electron cloud polarizability refers to how easily the electron cloud around an atom or a molecule can be distorted to form instantaneous dipoles. A polarizable electron cloud allows for a stronger interaction with other molecules through London dispersion forces.

Various factors influence electron cloud polarizability, including the number of electrons (linked to molar mass) and the overall volume of the electron cloud. More electrons mean a larger, more spread-out electron cloud that is easily distorted. Molecules with high polarizability therefore tend to have a higher boiling point as it takes more energy to disrupt these interactions. In our comparison between \( \mathrm{CO}_{2}(l) \) and \( \mathrm{CS}_{2}(l) \), the larger and more polarizable electron cloud of \( \mathrm{CS}_{2} \) contributes to its greater London dispersion forces compared to \( \mathrm{CO}_{2} \).