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Chapter 10: Problem 96

Table 10.3 shows that the van der Wals \(b\) parameter has units of L/mol. This means that we can calculate the sizes of atoms or molecules from the \(b\) parameter. Refer back to the discussion in Section \(7.3 .\) Is the van der Waals radius we calculate from the \(b\) parameter of Table 10.3 more closely associated with the bonding or nonbonding atomic radius discussed there? Explain.

Short Answer

Expert verified
The van der Waals radius, calculated from the $b$ parameter, is more closely associated with the nonbonding atomic radius. Both the van der Waals radius and the nonbonding atomic radius represent the distances between non-interacting atoms, excluding any significant interaction or attraction between them.

Step by step solution

01

Understanding van der Waals b parameter and its units

The van der Waals b parameter represents the volume occupied by one mole of molecules. It is a measure of the effective volume of the molecules themselves, excluding the interaction between them. The parameter has units of L/mol (liters per mole).
02

Relating van der Waals b parameter to atomic sizes

To calculate the sizes of atoms or molecules, we can use the van der Waals b parameter. We can assume that the van der Waals radius is half the distance between two molecules when they are at their closest approach, without significant interaction between them. By knowing the volume occupied by one mole of such molecules, we can determine their effective sizes.
03

Bonding and nonbonding atomic radii

In Section 7.3, two types of atomic radii were discussed: bonding and nonbonding atomic radii. The bonding atomic radius is the distance between the nuclei of two atoms when they are joined together, while the nonbonding atomic radius is the distance between the nuclei of two non-interacting atoms.
04

Comparing van der Waals radius with bonding and nonbonding atomic radii

The van der Waals radius is calculated by considering the volume occupied by one mole of non-interacting molecules. This radius is based on the closest approach between these molecules, excluding any significant interaction or attraction between them. Therefore, the van der Waals radius is more closely associated with the nonbonding atomic radius, as it also represents the distances between non-interacting atoms, rather than those involved in bonding.

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Most popular questions from this chapter

Which of the following statements best explains why a closed balloon filled with helium gas rises in air? \begin{equation}\begin{array}{l}{\text { (a) Helium is a monatomic gas, whereas nearly all the molecules }} \\ {\text { that make up air, such as nitrogen and oxygen, are }} \\ {\text { diatomic. }} \\ {\text { (b) The average speed of helium atoms is greater than the }} \\ {\text { average speed of air molecules, and the greater speed }} \\ {\text { of collisions with the balloon walls propels the balloon }} \\ {\text { upward. }}\\\\{\text { (c) Because the helium atoms are of lower mass than the average }} \\ {\text { air molecule, the helium gas is less dense than air. }} \\\ {\text { The mass of the balloon is thus less than the mass of the }} \\\ {\text { air displaced by its volume. }}\\\\{\text { (d) Because helium has a lower molar mass the average }} \\ {\text { air molecule, the helium atoms are in faster motion. This }} \\ {\text { means that the temperature of the helium is greater than }} \\ {\text { the air temperature. Hot gases tend to rise. }}\end{array} \end{equation}

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