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Ch.22 - The Main Group Elements
McMurry - Chemistry 8th Edition
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All textbooksMcMurry 8th EditionCh.22 - The Main Group ElementsProblem 22.133a
Chapter 22, Problem 22.133a

Write a balanced net ionic equation for the reaction of the amphoteric oxide Ga2O3 with:
a. Aqueous sulfuric acid

Verified step by step guidance
1
Identify the reactants: Gallium(III) oxide (Ga_2O_3) and sulfuric acid (H_2SO_4).
Write the balanced molecular equation for the reaction: Ga_2O_3 + 3H_2SO_4 → 2Ga^3+ + 3SO_4^2- + 3H_2O.
Separate the aqueous compounds into their respective ions: Ga_2O_3 (s) + 6H^+ (aq) + 3SO_4^2- (aq) → 2Ga^3+ (aq) + 3SO_4^2- (aq) + 3H_2O (l).
Cancel out the spectator ions (SO_4^2-) that appear on both sides of the equation.
Write the net ionic equation: Ga_2O_3 (s) + 6H^+ (aq) → 2Ga^3+ (aq) + 3H_2O (l).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Amphoteric Oxides

Amphoteric oxides are metal oxides that can react with both acids and bases. They exhibit dual behavior, meaning they can either donate or accept protons depending on the nature of the reacting substance. For example, gallium oxide (Ga2O3) can react with acids to form salts and with bases to form complex ions, showcasing its amphoteric nature.
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Amphoteric Species

Net Ionic Equations

A net ionic equation represents the chemical species that are actually involved in a reaction, omitting the spectator ions that do not participate. To write a net ionic equation, one must first write the balanced molecular equation, then dissociate the soluble ionic compounds into their constituent ions, and finally eliminate the spectator ions to focus on the species that undergo a change.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, sulfuric acid (H2SO4) acts as a strong acid, donating protons to the amphoteric oxide Ga2O3. Understanding the behavior of acids and bases, including their strength and the resulting products, is crucial for predicting the outcome of the reaction and writing the correct net ionic equation.
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Related Practice
Textbook Question

Using the shorthand notation of Figure 22.9, draw the structure of the silicate anion in:

(a) K4SiO4 (b) Ag10Si4O13

What is the relationship between the charge on the anion and the number of terminal O atoms?

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Textbook Question

An important physiological reaction of nitric oxide (NO) is its interaction with the superoxide ion (O2–) to form the peroxynitrite ion (ONOO–).

a. Write electron-dot structures for NO, O2–, and ONOO–, and predict the O–N–O bond angle in ONOO–.

101
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Textbook Question

Consider the six second- and third-row elements in groups 4A–6A of the periodic table:


Possible structures for the binary fluorides of each of these elements in its highest oxidation state are shown below.


(a) Identify the nonfluorine atom in each case, and write the molecular formula of each fluoride.

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Textbook Question

Write a balanced net ionic equation for the reaction of the amphoteric oxide ZnO with:

a. Hydrochloric acid

84
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Textbook Question

The following pictures represent various silicate anions. Write the formula and charge of each anion.

97
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Textbook Question

In the following pictures of binary hydrides, ivory spheres

represent H atoms or ions, and burgundy spheres represent

atoms or ions of the other element.

(1)

(2)

(3)

(4)

(a) Identify each binary hydride as ionic, covalent, or interstitial.

(b) What is the oxidation state of hydrogen in compounds (1), (2), and (3)? What is the oxidation state of the other

element?

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