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Chapter 12: Problem 178

Describe at the molecular level what is happening when solid iodine, \(\mathrm{I}_{2}(s)\), dissolves in carbon tetrachloride liquid, \(\operatorname{CCl}_{4}(l)\).

Short Answer

Expert verified
When solid iodine (I₂) dissolves in carbon tetrachloride (CCl₄), the nonpolar nature of both substances allows for weak London dispersion forces to form between their molecules. These forces overcome the van der Waals forces present in the crystalline structure of solid iodine, allowing I₂ molecules to diffuse into the CCl₄ liquid, resulting in a homogeneous solution.

Step by step solution

01

Identify the molecules involved

We have two substances: solid iodine (I₂) and carbon tetrachloride (CCl₄) liquid. Iodine is a diatomic molecule, meaning that it consists of two iodine atoms bonded together. Carbon tetrachloride is a molecular compound formed by a carbon atom (C) bonded to four chlorine atoms (Cl) in a tetrahedral shape.
02

Understand the initial state of solid iodine

Solid iodine has a crystalline structure where the individual I₂ molecules are held together by van der Waals forces (weak intermolecular forces). Each I₂ molecule consists of two iodine atoms covalently bonded together, forming a single I-I bond.
03

Consider the polarity of both substances

Since iodine (I₂) is a diatomic molecule, it is nonpolar in nature as there is no difference in electronegativity between the iodine atoms. Carbon tetrachloride (CCl₄) is also a nonpolar molecule due to its symmetrical structure that leads to equal distribution of electron density, even though the C-Cl bond itself is polar.
04

Understand the interactions between iodine and carbon tetrachloride molecules

As both iodine and carbon tetrachloride are nonpolar, there will be no formation of ion-dipole or dipole-dipole interactions between the molecules. Instead, the weak van der Waals forces, specifically London dispersion forces, will be responsible for holding I₂ and CCl₄ molecules together when mixed.
05

Describe the dissolving process of iodine in carbon tetrachloride

When solid iodine comes into contact with carbon tetrachloride, the London dispersion forces between the I₂ molecules and the CCl₄ molecules overcome the attractions within the I₂ solid lattice structure, allowing for individual I₂ molecules to diffuse into the CCl₄ liquid. The weak intermolecular forces between the I₂ and CCl₄ molecules allow I₂(s) to dissolve in CCl₄(l), resulting in a homogeneous solution.

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Most popular questions from this chapter

Suppose \(200.0 \mathrm{~mL}\) of a \(2.50 \mathrm{M}\) solution of sodium hydroxide is combined with \(100.0 \mathrm{~mL}\) of a \(1.50 \mathrm{M}\) solution of iron(III) nitrate. (a) Write a net ionic equation for the formation of the expected precipitate. (b) What is the theoretical yield of precipitate in grams? (c) Suppose only \(10.95 \mathrm{~g}\) of precipitate is isolated. What is the percent yield for the reaction? (d) What is the molar concentration of the excess reactant in the combined solution?

A solution of a particular solid solute in water has a concentration of \(25.0\) mass \(\%\). (a) Given \(100.0 \mathrm{~g}\) of this solution, how many grams of solute do you have? (b) Given \(48.0 \mathrm{~g}\) of this solution, how many grams of solute do you have? (c) How many grams of this solution do you need to obtain \(56.5 \mathrm{~g}\) of solute?

Carbon dioxide, \(\mathrm{CO}_{2}\), is a compound of carbon and oxygen. Does this mean that a sample of pure carbon dioxide can be considered to be a solution of carbon dissolved in oxygen? Explain your answer.

Which would you expect to release the most hydration energy when dissolved in water: \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(\mathrm{I}), \mathrm{CH}_{3} \mathrm{Cl}(l)\), or \(\mathrm{C}_{8} \mathrm{H}_{18}(I) ?\) Which would you expect to release the least hydration energy? Explain your answers.

Define vapor pressure and include the word equilibrium in your definition.
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