Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: FeO(s) + 2 HClO₄(aq) → Fe(ClO₄)₂(aq) + H₂O(l) (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between NiO(s) and an aqueous solution of nitric acid.

Verified step by step guidance

1. Identify the reactants: Nickel(II) oxide (NiO) and nitric acid (HNO₃).
2. Write the balanced molecular equation for the reaction: NiO(s) + 2HNO₃(aq) → Ni(NO₃)₂(aq) + H₂O(l).
3. Determine the ions present in the aqueous solution: H⁺ and NO₃⁻ from HNO₃, and Ni²⁺ and NO₃⁻ from Ni(NO₃)₂.
4. Identify the spectator ions: NO₃⁻ ions are present on both sides of the equation and do not participate in the reaction.
5. Write the net ionic equation by removing the spectator ions: NiO(s) + 2H⁺(aq) → Ni²⁺(aq) + H₂O(l).

Key Concepts

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, metal oxides, which are basic, react with acids to form water and a salt. Understanding the nature of acids and bases, as defined by the Brønsted-Lowry theory, is crucial for predicting the products of such reactions.

Net Ionic Equations

A net ionic equation represents the actual chemical species that are involved in a reaction, excluding spectator ions that do not participate. To write a net ionic equation, one must first identify the reactants and products, then eliminate ions that appear unchanged on both sides of the equation, focusing on the species that undergo a change.

Metal Oxides

Metal oxides are compounds formed by the reaction of metals with oxygen, typically exhibiting basic properties. When metal oxides like NiO react with acids, they neutralize the acid, leading to the formation of water and a corresponding salt. Recognizing the behavior of metal oxides in acid-base chemistry is essential for understanding their reactivity.