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Chapter 3: Problem 6

Write dissociation equations for the following ionic compounds. a. \(\mathrm{LiF}(s)\) b. \(\mathrm{CuSO}_{4}(s)\) c. \(\mathrm{Na}_{2} \mathrm{~S}(s)\) d. \(\mathrm{MgBr}_{2}(s)\)

Short Answer

Expert verified
LiF: \(\mathrm{LiF}(s) \rightarrow \mathrm{Li^+}(aq) + \mathrm{F^-}(aq)\); CuSO4: \(\mathrm{CuSO}_{4}(s) \rightarrow \mathrm{Cu^{2+}}(aq) + \mathrm{SO}_{4}^{2-}(aq)\); Na2S: \(\mathrm{Na}_{2} \mathrm{~S}(s) \rightarrow 2\mathrm{Na^+}(aq) + \mathrm{S}^{2-}(aq)\); MgBr2: \(\mathrm{MgBr}_{2}(s) \rightarrow \mathrm{Mg^{2+}}(aq) + 2\mathrm{Br^-}(aq)\).

Step by step solution

01

Understanding Dissociation

The process of dissociation involves breaking down an ionic compound into its constituent ions when dissolved in water. Solid compounds (denoted by (s)) will dissociate into their respective positive (cations) and negative ions (anions) in aqueous solutions (denoted by (aq)).
02

Dissociate LiF

The compound lithium fluoride (\(\mathrm{LiF}(s)\)) dissociates into lithium ions \(\mathrm{Li^+}(aq)\) and fluoride ions \(\mathrm{F^-}(aq)\) when dissolved in water. The dissociation equation is: \(\mathrm{LiF}(s) \rightarrow \mathrm{Li^+}(aq) + \mathrm{F^-}(aq)\).
03

Dissociate CuSO4

Copper(II) sulfate (\(\mathrm{CuSO}_{4}(s)\)) dissociates into copper(II) ions \(\mathrm{Cu^{2+}}(aq)\) and sulfate ions \(\mathrm{SO}_{4}^{2-}(aq)\). The dissociation equation is: \(\mathrm{CuSO}_{4}(s) \rightarrow \mathrm{Cu^{2+}}(aq) + \mathrm{SO}_{4}^{2-}(aq)\).
04

Dissociate Na2S

Sodium sulfide (\(\mathrm{Na}_{2} \mathrm{~S}(s)\)) dissociates into two sodium ions \(2\mathrm{Na^+}(aq)\) and one sulfide ion \(\mathrm{S}^{2-}(aq)\). The dissociation equation is: \(\mathrm{Na}_{2} \mathrm{~S}(s) \rightarrow 2\mathrm{Na^+}(aq) + \mathrm{S}^{2-}(aq)\).
05

Dissociate MgBr2

Magnesium bromide (\(\mathrm{MgBr}_{2}(s)\)) dissociates into one magnesium ion \(\mathrm{Mg^{2+}}(aq)\) and two bromide ions \(2\mathrm{Br^-}(aq)\). The dissociation equation is: \(\mathrm{MgBr}_{2}(s) \rightarrow \mathrm{Mg^{2+}}(aq) + 2\mathrm{Br^-}(aq)\).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Ions in Aqueous Solutions
When ionic compounds dissolve in water, they separate into individual ions. This process is crucial in chemistry because it determines how substances interact in a solution. Consider the compound lithium fluoride (LiF): in its solid state, the ions are tightly packed together. Upon adding it to water, the LiF breaks apart, releasing lithium ions (\(\mathrm{Li^+} \text{(aq)}\)) and fluoride ions (\(\mathrm{F^-} \text{(aq)}\)).

In an aqueous solution, ions facilitate various chemical reactions and processes.
For instance, they can:
  • Conduct electricity, as free-moving charged particles carry current.
  • Participate in precipitations, like when solutions are mixed and a solid forms.
  • Engage in oxidation-reduction reactions, transferring electrons between species.
Understanding ions in solution is fundamental to predicting the behavior of chemicals in water.
Dissociation of Ionic Compounds
Dissociation refers to the separation of molecules into smaller particles, particularly ions, when dissolved. Ionic compounds, built from positive and negative ions, readily dissociate in water. Take copper(II) sulfate (CuSO鈧�) as an example; it consists of copper ions (Cu虏鈦�) and sulfate ions (SO鈧劼测伝).

When CuSO鈧� is introduced into water, its formula changes into Cu虏鈦�(aq) and SO鈧劼测伝(aq). This involves:
  • The surrounding water molecules separating the individual ions.
  • Energetic processes where bonds between ions break and new interactions with water form.
Highlighting dissociation equations can help recognize distinct ions present in the solution, essential for calculating reaction stoichiometry and understanding solubility.
Chemical Reactions in Water
Chemical reactions in water are defined by the interactions of dissolved ions. When ionic substances such as magnesium bromide (MgBr鈧�) enter water, they dissociate into their respective ions, Mg虏鈦�(aq) and 2Br鈦�(aq). This prepares them to participate in potential chemical transformations.

Key features of reactions involving dissolved ions include:
  • Precipitation reactions where two solutions mix, and an insoluble salt forms.
  • Acid-base reactions which involve hydrogen ion (H鈦�) transfer between reactants.
  • Redox reactions that see the exchange of electrons.
In all these processes, water serves as a solvent, allowing ions to move freely, collide, and react. Comprehending how chemical reactions proceed in aqueous environments is crucial in fields ranging from biological systems to industrial processes.

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Most popular questions from this chapter

Both tin and lead acquire \(2+\) or \(4+\) charges when they become ions. Use the periodic table to explain why this should not surprise you.

What is the formula mass for each compound? a. \(\mathrm{Co}\left(\mathrm{HCO}_{3}\right)_{2}\) b. \(\mathrm{LiHCO}_{3}\)

What are the two types of ions?

Write the chemical formula for the ionic compound formed by each pair of ions. a. \(\mathrm{Cr}^{3+}\) and \(\mathrm{O}^{2-}\) b. \(\mathrm{Cr}^{2+}\) and \(\mathrm{O}^{2-}\) c. \(\mathrm{Pb}^{2+}\) and \(\mathrm{Cl}^{-}\) d. \(\mathrm{Pb}^{4+}\) and \(\mathrm{Cl}^{-}\)

A calcium atom has two valence electrons. Do you think it will lose two electrons or gain six electrons to obtain an octet in its outermost electron shell? Write the formula of the resulting ion.
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