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Chapter 15: Problem 50

True or false? Because the solid phase of a molecular compound does not consist of ions, the compound cannot dissociate into ions when it dissolves in water. Back up your answer with an explanation and an example.

Short Answer

Expert verified
True. Molecular compounds, consisting of covalent bonds between non-metal atoms, do not dissociate into ions when dissolved in water. Instead, they dissolve as entire molecules. For example, when sugar (C12H22O11) dissolves in water, the molecules remain intact and disperse throughout the water, creating a homogeneous mixture, but they do not dissociate into ions.

Step by step solution

01

Define dissociation and molecular compounds

Dissociation is the process by which a compound breaks apart into its constituent ions when dissolved in a solvent, typically water. It's important for understanding solubility and the behavior of compounds in aqueous solutions. Molecular compounds consist of molecules formed by covalent bonding between non-metal atoms. These compounds do not contain ions, unlike ionic compounds, which comprise a lattice structure of positively and negatively charged ions.
02

Determine the statement's validity

The statement is true. Because the solid phase of a molecular compound does not consist of ions, indeed the compound cannot dissociate into ions when it dissolves in water.
03

Provide an explanation

Molecular compounds contain covalent bonds, where electrons are shared between atoms, rather than transferred as in ionic compounds. When dissolving in water, these bonds might weaken, but the compound will not dissociate into individual ions. Instead, they will dissolve as entire molecules. This is different from ionic compounds, where the ions separate in the solution, forming a mixture of free cations and anions.
04

Present an example

A good example of a molecular compound that does not dissociate into ions when dissolved in water is sugar (sucrose, C12H22O11). When sugar dissolves in water, its covalent bonds are not broken, and it does not form ions. The sugar molecules remain intact and simply disperse throughout the water, creating a homogeneous mixture.

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Most popular questions from this chapter

If \(0.378 \mathrm{~g}\) of HBr dissolved in enough water to make \(1.25 \mathrm{~L}\) of solution, what is the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration? What is the \(\mathrm{OH}^{-}\) concentration?

Without using a calculator, what is the base-10 logarithm of \(10^{13}\) ?

The pH of a solution is \(-1\). What are the \(\mathrm{H}_{3} \mathrm{O}^{+}\) and OH concentrations? Is the solution acidic or basic?

Acrylic acid, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{COOH}\), is a weak monoprotic acid. Write a balanced equation for the reaction that occurs when \(25.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{KOH}\) is added to \(50.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{COOH}\). Besides water, what species are present in the solution? Is this solution a buffer? Why or why not?

Suppose \(2.0\) moles of sodium acetate, \(\mathrm{NaO}_{2} \mathrm{CCH}_{3}\), are dissolved in some water and then \(1.0 \mathrm{~L}\) of a \(1.0 \mathrm{M} \mathrm{HCl}\) solution is added. (a) Write the chemical reaction that occurs. (b) After the reaction, what are the predominant species in solution? How many moles of each species are there? (c) Is the resulting solution a buffer? If yes, explain why.
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