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

Verified step by step guidance

1. Identify the ions present in the compound K₂O. Potassium oxide (K₂O) consists of potassium ions (K⁺) and oxide ions (O²⁻).
2. Recall the solubility rules for ionic compounds in water. One key rule is that all compounds containing alkali metal ions (such as K⁺) are soluble in water.
3. Since K₂O contains potassium ions, which are alkali metal ions, apply the solubility rule that states compounds with alkali metal ions are soluble.
4. Consider the oxide ion (O²⁻). While many oxides are not soluble, the presence of the alkali metal ion (K⁺) takes precedence according to the solubility rules.
5. Conclude that K₂O is soluble in water due to the presence of the potassium ion, an alkali metal ion, which makes the compound soluble.

Key Concepts

Ionic Compounds

Ionic compounds are formed from the electrostatic attraction between positively and negatively charged ions. They typically consist of a metal and a non-metal, where the metal donates electrons to the non-metal, resulting in the formation of cations and anions. Understanding the nature of these compounds is essential for predicting their solubility in water.

Solubility Rules

Solubility rules are guidelines that help predict whether an ionic compound will dissolve in water. These rules indicate that most alkali metal compounds, such as those containing potassium (K), are soluble in water. Familiarity with these rules is crucial for determining the solubility of specific ionic compounds like K₂O.

Hydration of Ions

Hydration of ions refers to the process where water molecules surround and interact with ions in a solution. This interaction stabilizes the ions and allows them to disperse in the solvent, leading to solubility. For K₂O, the potassium ions (K⁺) and oxide ions (O²⁻) will undergo hydration, influencing the overall solubility of the compound in water.