Write a balanced net ionic equation for the reaction of each of the following oxides with water: (a) BaO (b) Cs2O (c) N2O5.

Verified step by step guidance

1. Identify the type of oxide: Determine whether each oxide is a basic oxide (metal oxide) or an acidic oxide (non-metal oxide). BaO and Cs2O are basic oxides, while N2O5 is an acidic oxide.
2. Write the reaction with water: For basic oxides, the reaction with water forms a metal hydroxide. For acidic oxides, the reaction with water forms an acid. Write the chemical equation for each reaction: (a) BaO + H2O -> Ba(OH)2, (b) Cs2O + H2O -> 2 CsOH, (c) N2O5 + H2O -> 2 HNO3.
3. Dissociate strong electrolytes: Identify strong electrolytes in the products and dissociate them into their respective ions. For example, Ba(OH)2 dissociates into Ba^{2+} and 2 OH^{-}.
4. Write the complete ionic equation: Express each reaction in terms of ions, showing all soluble ionic compounds as dissociated ions. For example, BaO + H2O -> Ba^{2+} + 2 OH^{-}.
5. Cancel spectator ions: Identify and cancel out ions that appear on both sides of the equation to write the net ionic equation. For example, if there are no spectator ions, the net ionic equation is the same as the complete ionic equation.

Key Concepts

Net Ionic Equations

A net ionic equation represents the chemical species that are involved in a reaction, excluding spectator ions. It highlights the actual chemical change occurring in a solution, focusing on the ions and molecules that participate directly in the reaction. This simplification is crucial for understanding the underlying chemistry, especially in aqueous reactions.

Oxides and Their Reactions with Water

Oxides are compounds formed by the reaction of an element with oxygen. When certain oxides react with water, they can form either acids or bases, depending on their nature. For example, metal oxides typically produce basic solutions, while non-metal oxides often yield acidic solutions, which is essential for predicting the products of the reactions in the question.

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of atoms for each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Proper balancing is crucial for accurately representing the stoichiometry of the reaction and for deriving the correct net ionic equation.