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Ch.22 - Chemistry of the Nonmetals
All textbooksBrown 14th EditionCh.22 - Chemistry of the NonmetalsProblem 39
Chapter 22, Problem 39

Complete the exercises below. Predict whether each of the following oxides is acidic, basic, amphoteric, or neutral: a. NO₂, b. CO₂, c. Al₂O₃, d. CaO.

Verified step by step guidance
1
Step 1: Understand the nature of oxides. Oxides can be classified as acidic, basic, amphoteric, or neutral based on their chemical behavior with water and acids/bases.
Step 2: Analyze the oxide NO₂. Nitrogen is a non-metal, and non-metal oxides typically form acidic oxides. Consider how NO₂ reacts with water to form an acid.
Step 3: Analyze the oxide CO₂. Carbon is a non-metal, and CO₂ is known to react with water to form carbonic acid, indicating it is an acidic oxide.
Step 4: Analyze the oxide Al₂O₃. Aluminum is a metal, but Al₂O₃ is known to react with both acids and bases, which is characteristic of amphoteric oxides.
Step 5: Analyze the oxide CaO. Calcium is a metal, and metal oxides typically form basic oxides. Consider how CaO reacts with water to form a base.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acidic and Basic Oxides

Oxides can be classified based on their behavior in reactions with acids and bases. Acidic oxides, such as CO₂, react with bases to form salts and water, while basic oxides, like CaO, react with acids to produce salts and water. This classification is essential for predicting the nature of the oxides in the given question.
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Amphoteric Oxides

Amphoteric oxides can react with both acids and bases, exhibiting dual behavior. An example is Al₂O₃, which can react with hydrochloric acid to form aluminum chloride and with sodium hydroxide to form sodium aluminate. Understanding this property is crucial for determining the classification of certain oxides.
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Neutral Oxides

Neutral oxides do not exhibit acidic or basic properties and do not react with either acids or bases. Examples include gases like NO, which do not form salts with acids or bases. Recognizing neutral oxides helps in accurately predicting the behavior of the oxides listed in the question.
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Related Practice
Textbook Question

Write balanced equations for each of the following reactions.

b. When copper(II) nitrate is heated strongly, it decomposes to form copper(II) oxide, nitrogen dioxide, and oxygen.

e. Potassium peroxide reacts with CO2(g) to give potassium carbonate and O2.