Textbook Question
Draw the electron-dot structure for CO, CO2, and CO32–, and predict which substance will have the strongest carbon–oxygen bond.
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Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 22, Problem 22.9
Which of the following oxides will be more soluble in acidic solution? (LO 22.14)
(a) SiO2 (b) NO2
(c) BaO (d) B2O3
Verified step by step guidance1
Identify the nature of each oxide: acidic, basic, or amphoteric.
Recall that basic oxides are more soluble in acidic solutions due to acid-base reactions.
Determine the nature of each oxide: SiO2 is acidic, NO2 is acidic, BaO is basic, and B2O3 is acidic.
Recognize that BaO, being a basic oxide, will react with an acidic solution to form a salt and water.
Conclude that BaO will be more soluble in an acidic solution compared to the other oxides.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Acid-Base Reactions
Acid-base reactions involve the transfer of protons (H+) between reactants. In the context of oxides, acidic solutions can react with basic oxides to form soluble salts and water. Understanding the nature of the oxide—whether it behaves as an acid or a base—helps predict its solubility in acidic conditions.
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Acid-Base Reaction
Solubility of Metal Oxides
The solubility of metal oxides in acidic solutions often depends on the metal's oxidation state and the oxide's basicity. Basic oxides, such as BaO, typically react with acids to form soluble salts, while amphoteric oxides, like B2O3, can react with both acids and bases, influencing their solubility in acidic environments.
Amphoteric Behavior
Amphoteric oxides can react with both acids and bases, exhibiting dual behavior. For example, B2O3 can dissolve in acidic solutions, while SiO2 is generally considered insoluble. Recognizing which oxides are amphoteric is crucial for determining their solubility in acidic conditions.
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03:03Amphoteric Species
Related Practice
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Compare and contrast the properties of ammonia and phosphine.
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GeCl4 reacts with Cl- to give GeCl62-, but CCl4 does not react with excess Cl-. Explain.
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In what forms is oxygen commonly found in nature?
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Describe the structures of the white and red allotropes of phosphorus, and explain why white phosphorus is so reactive.
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Which of the following elements (X) will form a covalent hydride with the formula XH3 that is a gas at room temperature? (LO 22.4)
(a) Al (b) As (c) Ba (d) Se
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