Which Of The Following Is Predicted To Have The Lowest Boiling Point?A. I 2 I_2 I 2 ​ B. C S 2 CS_2 C S 2 ​ C. C C L 4 CCl_4 CC L 4 ​ D. C B R 4 CBr_4 CB R 4 ​

Introduction

In chemistry, the boiling point of a substance is a critical property that determines its physical state at a given temperature. The boiling point is the temperature at which a liquid transforms into a gas. In this article, we will discuss the boiling points of four compounds: $I_2$, $CS_2$, $CCl_4$, and $CBr_4$. We will analyze the intermolecular forces present in these compounds and predict which one has the lowest boiling point.

Intermolecular Forces

Intermolecular forces are the attractive and repulsive forces between molecules. These forces play a crucial role in determining the physical properties of a substance, including its boiling point. The strength of intermolecular forces depends on the type of molecules and the nature of the intermolecular interactions.

London Dispersion Forces

London dispersion forces are a type of intermolecular force that arises due to temporary dipoles in nonpolar molecules. These forces are weak and increase with the size of the molecule. The larger the molecule, the stronger the London dispersion forces.

Dipole-Dipole Forces

Dipole-dipole forces are a type of intermolecular force that arises due to the interaction between two polar molecules. These forces are stronger than London dispersion forces and increase with the magnitude of the dipole moment.

Hydrogen Bonding

Hydrogen bonding is a type of intermolecular force that arises due to the interaction between a hydrogen atom bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) and another electronegative atom. These forces are strong and play a crucial role in determining the physical properties of substances.

Boiling Points of the Compounds

Now, let's analyze the boiling points of the four compounds: $I_2$, $CS_2$, $CCl_4$, and $CBr_4$.

$I_2$

$I_2$ is a nonpolar molecule with a large molecular size. The London dispersion forces present in this molecule are strong due to its large size. The boiling point of $I_2$ is 458.4 K.

$CS_2$

$CS_2$ is a polar molecule with a dipole moment of 1.98 D. The dipole-dipole forces present in this molecule are moderate due to its polar nature. The boiling point of $CS_2$ is 319.4 K.

$CCl_4$

$CCl_4$ is a nonpolar molecule with a large molecular size. The London dispersion forces present in this molecule are strong due to its large size. The boiling point of $CCl_4$ is 350.9 K.

$CBr_4$

$CBr_4$ is a nonpolar molecule with a large molecular size. The London dispersion forces present in this molecule are strong due to its large size. The boiling point of $CBr_4$ is 414.6 K.

Prediction

Based on the analysis of the intermolecular forces present in the four compounds, we can predict that $CS_2$ has the lowest boiling point. The dipole-dipole forces present in $CS_2$ are moderate, which results in a lower boiling point compared to the other three compounds.

Conclusion

In conclusion, the boiling point of a substance is a critical property that determines its physical state at a given temperature. The intermolecular forces present in a substance play a crucial role in determining its boiling point. By analyzing the intermolecular forces present in the four compounds: $I_2$, $CS_2$, $CCl_4$, and $CBr_4$, we can predict that $CS_2$ has the lowest boiling point.

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.
• Levine, I. N. (2012). Physical chemistry (6th ed.). McGraw-Hill.

Table of Boiling Points

Compound	Boiling Point (K)
$I_2$	458.4
$CS_2$	319.4
$CCl_4$	350.9
$CBr_4$	414.6

Comparison of Boiling Points

Compound	Boiling Point (K)	Difference (K)
$I_2$	458.4	139.0
$CS_2$	319.4	0.0
$CCl_4$	350.9	31.5
$CBr_4$	414.6	95.2

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Introduction

In our previous article, we discussed the boiling points of four compounds: $I_2$, $CS_2$, $CCl_4$, and $CBr_4$. We analyzed the intermolecular forces present in these compounds and predicted that $CS_2$ has the lowest boiling point. In this article, we will answer some frequently asked questions related to the boiling points of these compounds.

Q: What are the main factors that affect the boiling point of a substance?

A: The main factors that affect the boiling point of a substance are the intermolecular forces present in the substance. These forces can be London dispersion forces, dipole-dipole forces, or hydrogen bonding.

Q: What are London dispersion forces?

A: London dispersion forces are a type of intermolecular force that arises due to temporary dipoles in nonpolar molecules. These forces are weak and increase with the size of the molecule.

Q: What are dipole-dipole forces?

A: Dipole-dipole forces are a type of intermolecular force that arises due to the interaction between two polar molecules. These forces are stronger than London dispersion forces and increase with the magnitude of the dipole moment.

Q: What are hydrogen bonding?

A: Hydrogen bonding is a type of intermolecular force that arises due to the interaction between a hydrogen atom bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) and another electronegative atom. These forces are strong and play a crucial role in determining the physical properties of substances.

Q: Why does $CS_2$ have the lowest boiling point among the four compounds?

A: $CS_2$ has the lowest boiling point among the four compounds because it has the weakest intermolecular forces. The dipole-dipole forces present in $CS_2$ are moderate, which results in a lower boiling point compared to the other three compounds.

Q: What is the boiling point of $I_2$?

A: The boiling point of $I_2$ is 458.4 K.

Q: What is the boiling point of $CCl_4$?

A: The boiling point of $CCl_4$ is 350.9 K.

Q: What is the boiling point of $CBr_4$?

A: The boiling point of $CBr_4$ is 414.6 K.

Q: Can you compare the boiling points of the four compounds?

A: Yes, the boiling points of the four compounds are:

Compound	Boiling Point (K)
$I_2$	458.4
$CS_2$	319.4
$CCl_4$	350.9
$CBr_4$	414.6

Q: What is the difference in boiling points between $I_2$ and $CS_2$?

A: The difference in boiling points between $I_2$ and $CS_2$ is 139.0 K.

Q: What is the difference in boiling points between $CCl_4$ and $CS_2$?

A: The difference in boiling points between $CCl_4$ and $CS_2$ is 31.5 K.

Q: What is the difference in boiling points between $CBr_4$ and $CS_2$?

A: The difference in boiling points between $CBr_4$ and $CS_2$ is 95.2 K.

Conclusion

In conclusion, the boiling points of substances are affected by the intermolecular forces present in the substance. By analyzing the intermolecular forces present in the four compounds: $I_2$, $CS_2$, $CCl_4$, and $CBr_4$, we can predict that $CS_2$ has the lowest boiling point. We hope that this Q&A article has provided you with a better understanding of the boiling points of these compounds.

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.
• Levine, I. N. (2012). Physical chemistry (6th ed.). McGraw-Hill.