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Ch.9 Solutions
Timberlake - Chemistry: An Introduction to General, Organic, and Biological Chemistry 13th Edition
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Capitolo 9, Problema 31d

Predict whether each of the following ionic compounds is soluble in water:
d. K2O

Guida verificata passo dopo passo
1
Identify the ions that make up the compound K₂O. Potassium (K⁺) is a Group 1 metal, and oxygen (O²⁻) is the anion.
Recall the solubility rules for ionic compounds. One key rule is that all compounds containing Group 1 metal cations (such as K⁺) are soluble in water.
Apply the solubility rule to K₂O. Since it contains the Group 1 metal potassium (K⁺), the compound is expected to be soluble in water.
Consider any exceptions to the solubility rules. In this case, there are no exceptions that apply to K₂O, so the compound remains soluble.
Conclude that K₂O is soluble in water based on the solubility rules and the absence of exceptions.

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Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively and negatively charged ions. These compounds typically consist of a metal and a non-metal, and their properties include high melting and boiling points, as well as electrical conductivity when dissolved in water.
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Naming Ionic Compounds

Solubility Rules

Solubility rules are guidelines that help predict whether an ionic compound will dissolve in water. Common rules include that most alkali metal compounds and nitrates are soluble, while many carbonates and phosphates are not. Understanding these rules is essential for determining the solubility of specific compounds.
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Solubility Rules

Potassium Oxide (K₂O)

Potassium oxide (K₂O) is an ionic compound formed from potassium ions (K⁺) and oxide ions (O²⁻). According to solubility rules, compounds containing alkali metals, such as potassium, are generally soluble in water. Therefore, K₂O is expected to react with water to form potassium hydroxide (KOH), which is soluble.
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Calculate Oxidation Numbers
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