Intermolecular Forces and Freezing Point

Oct 13, 2025 by thesweetdesigns.com 124 views

Introduction

In chemistry, the freezing point of a substance is the temperature at which it changes state from a liquid to a solid. The freezing point is an important property of a substance, and it is influenced by the intermolecular forces between the molecules of the substance. In this article, we will discuss which of the following substances has the lowest freezing point: H₂O (water), N₂ (nitrogen), SO₂ (sulfur dioxide), H₂ (hydrogen), and CO₂ (carbon dioxide).

Intermolecular Forces and Freezing Point

The freezing point of a substance is directly related to the strength of the intermolecular forces between its molecules. Substances with strong intermolecular forces have higher freezing points, while substances with weak intermolecular forces have lower freezing points. There are several types of intermolecular forces, including:

London dispersion forces: These are weak forces that arise from the temporary dipoles that form in nonpolar molecules.
Dipole-dipole forces: These are forces that arise from the attraction between two polar molecules.
Hydrogen bonding: This is a type of dipole-dipole force that occurs between molecules that have a hydrogen atom bonded to a highly electronegative atom, such as oxygen, nitrogen, or fluorine.

Analysis of the Options

Now, let's analyze each of the options to determine which one has the lowest freezing point.

A. H₂O (Water)

Water is a polar molecule that exhibits hydrogen bonding. The hydrogen bonding in water is strong, which results in a high freezing point of 0°C (32°F) at standard pressure.

B. N₂ (Nitrogen)

Nitrogen is a nonpolar molecule that exhibits only London dispersion forces. The London dispersion forces in nitrogen are weak, which results in a very low freezing point of -209.86°C (-345.75°F) at standard pressure.

C. SO₂ (Sulfur Dioxide)

Sulfur dioxide is a polar molecule that exhibits dipole-dipole forces. The dipole-dipole forces in sulfur dioxide are moderate, which results in a freezing point of -72.73°C (-98.01°F) at standard pressure.

D. H₂ (Hydrogen)

Hydrogen is a nonpolar molecule that exhibits only London dispersion forces. The London dispersion forces in hydrogen are weak, which results in a very low freezing point of -259.11°C (-434.40°F) at standard pressure.

E. CO₂ (Carbon Dioxide)

Carbon dioxide is a nonpolar molecule that exhibits only London dispersion forces. The London dispersion forces in carbon dioxide are weak, which results in a very low freezing point of -56.56°C (-69.81°F) at standard pressure.

Conclusion

Based on the analysis of the options, we can conclude that the substance with the lowest freezing point is D. H₂ (Hydrogen). The London dispersion forces in hydrogen are weak, which results in a very low freezing point of -259.11°C (-434.40°F) at standard pressure.

Comparison of Freezing Points

Here is a comparison of the freezing points of the five substances:

Substance	Freezing Point (°C)	Freezing Point (°F)
H₂O (Water)	0	32
N₂ (Nitrogen)	-209.86	-345.75
SO₂ (Sulfur Dioxide)	-72.73	-98.01
H₂ (Hydrogen)	-259.11	-434.40
CO₂ (Carbon Dioxide)	-56.56	-69.81

Key Takeaways

The freezing point of a substance is directly related to the strength of the intermolecular forces between its molecules.
Substances with strong intermolecular forces have higher freezing points, while substances with weak intermolecular forces have lower freezing points.
The substance with the lowest freezing point is H₂ (hydrogen), which has a freezing point of -259.11°C (-434.40°F) at standard pressure.

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Chang, R. (2010). Chemistry: The central science (11th ed.). McGraw-Hill.
Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2007). General chemistry: Principles and modern applications (9th ed.). Pearson Prentice Hall.
Q&A: Freezing Points and Intermolecular Forces =============================================

Introduction

In our previous article, we discussed the concept of freezing points and how they are related to the strength of intermolecular forces between molecules. We also analyzed the freezing points of five substances: H₂O (water), N₂ (nitrogen), SO₂ (sulfur dioxide), H₂ (hydrogen), and CO₂ (carbon dioxide). In this article, we will answer some frequently asked questions about freezing points and intermolecular forces.

Q: What is the relationship between freezing point and intermolecular forces?

A: The freezing point of a substance is directly related to the strength of the intermolecular forces between its molecules. Substances with strong intermolecular forces have higher freezing points, while substances with weak intermolecular forces have lower freezing points.

Q: What types of intermolecular forces are there?

A: There are several types of intermolecular forces, including:

London dispersion forces: These are weak forces that arise from the temporary dipoles that form in nonpolar molecules.
Dipole-dipole forces: These are forces that arise from the attraction between two polar molecules.
Hydrogen bonding: This is a type of dipole-dipole force that occurs between molecules that have a hydrogen atom bonded to a highly electronegative atom, such as oxygen, nitrogen, or fluorine.

Q: Why do some substances have very low freezing points?

A: Some substances have very low freezing points because they have weak intermolecular forces. For example, hydrogen (H₂) has a very low freezing point of -259.11°C (-434.40°F) at standard pressure because it has only London dispersion forces.

Q: Can you give an example of a substance with a high freezing point?

A: Yes, water (H₂O) is a substance with a high freezing point of 0°C (32°F) at standard pressure. This is because water has strong hydrogen bonding between its molecules.

Q: How do you determine the freezing point of a substance?

A: The freezing point of a substance can be determined by measuring the temperature at which it changes state from a liquid to a solid. This can be done using a thermometer or other temperature-measuring device.

Q: What is the significance of freezing points in everyday life?

A: Freezing points are significant in everyday life because they can affect the behavior of substances in various situations. For example, the freezing point of water is important for understanding the behavior of water in cold temperatures, while the freezing point of other substances can affect the behavior of materials in various applications.

Q: Can you give an example of a real-world application of freezing points?

A: Yes, the freezing point of water is important for understanding the behavior of water in cold temperatures, which is why it is used in various applications such as:

Ice skating: The freezing point of water is important for understanding the behavior of ice on a skating rink.
Ice fishing: The freezing point of water is important for understanding the behavior of ice on a frozen lake or river.
Food preservation: The freezing point of water is important for understanding the behavior of food in cold temperatures, which is why it is used in various applications such as freezing food for preservation.

Conclusion

In conclusion, freezing points and intermolecular forces are important concepts in chemistry that can affect the behavior of substances in various situations. By understanding the relationship between freezing points and intermolecular forces, we can better understand the behavior of substances in various applications.

Key Takeaways

The freezing point of a substance is directly related to the strength of the intermolecular forces between its molecules.
Substances with strong intermolecular forces have higher freezing points, while substances with weak intermolecular forces have lower freezing points.
The freezing point of a substance can be determined by measuring the temperature at which it changes state from a liquid to a solid.
Freezing points are significant in everyday life because they can affect the behavior of substances in various situations.

References

Atkins, P. W., & De Paula, J. (2010). Physical chemistry (9th ed.). Oxford University Press.
Chang, R. (2010). Chemistry: The central science (11th ed.). McGraw-Hill.
Petrucci, R. H., Harwood, W. S., & Herring, F. G. (2007). General chemistry: Principles and modern applications (9th ed.). Pearson Prentice Hall.