Question

Classify the following oxides as acidic, basic, amphoteric, (c) CaO, (e) CO, or neutral: (a) \(\mathrm{CO}_{2}\), (b) \(\mathrm{K}_{2} \mathrm{O}\) (d) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (f) \(\mathrm{NO},(\mathrm{g}) \mathrm{SnO}_{2},\) (i) \(\mathrm{Al}_{2} \mathrm{O}_{3},(\mathrm{j}) \mathrm{BaO}\) (h) \(\mathrm{SO}_{3}\)

Short answer

(a) Acidic, (b) Basic, (c) Basic, (d) Acidic, (e) Neutral, (f) Neutral, (g) Amphoteric, (h) Acidic, (i) Amphoteric, (j) Basic.

Step-by-step solution

Understanding Acidic Oxides

Acidic oxides are typically formed by nonmetals and react with water to form acids. Evaluate which of the given oxides fall into this category.

Assessing Basic Oxides

Basic oxides are usually formed by metals and react with water to form bases (alkalies). Identify the basic oxides from the list.

Identifying Amphoteric Oxides

Amphoteric oxides can react with both acids and bases to form salts and water. Recognize any oxides with mixed characteristics.

Classification of Each Oxide

Classify each given oxide:- (a) \(\mathrm{CO}_{2}\): Acidic oxide, as it forms carbonic acid in water.- (b) \(\mathrm{K}_{2} \mathrm{O}\): Basic oxide, as it forms potassium hydroxide in water.- (c) \(\mathrm{CaO}\): Basic oxide, as it forms calcium hydroxide in water.- (d) \(\mathrm{N}_{2} \mathrm{O}_{5}\): Acidic oxide, as it forms nitric acid in water.- (e) \(\mathrm{CO}\): Neutral oxide, as it doesn't react significantly with water.- (f) \(\mathrm{NO}\): Neutral oxide, due to its limited reaction with water.- (g) \(\mathrm{SnO}_{2}\): Amphoteric oxide, as it reacts with both acids and bases.- (h) \(\mathrm{SO}_{3}\): Acidic oxide, as it forms sulfuric acid in water.- (i) \(\mathrm{Al}_{2} \mathrm{O}_{3}\): Amphoteric oxide, as it reacts with both acids and bases.- (j) \(\mathrm{BaO}\): Basic oxide, as it forms barium hydroxide in water.

Key concepts

Acidic Oxides

Acidic oxides are compounds that typically consist of nonmetals bonded with oxygen. They have a unique ability to react with water, forming acids in the process. This characteristic is what gives them their name, as the resulting solutions from these reactions are acidic in nature. For instance, when carbon dioxide (

Basic Oxides

Basic oxides are formed when metals combine with oxygen. These oxides characteristically react with water to form bases, or alkaline solutions. This is the defining property that distinguishes them as basic oxides. Consider - Potassium oxide Basic oxides' ability to form alkaline solutions makes them crucial in applications like neutralizing acids in various chemical processes. Understanding the reactions that produce basic oxides helps in predicting their behavior when combined with water or other compounds.

Amphoteric Oxides

Amphoteric oxides are a special category, as they possess the unique ability to react with both acids and bases. This dual reactive nature allows them to form salts and water in different reactions, depending on what they are interacting with. Oxides like - Tin oxide (SnO - Aluminum oxide ( Amphoteric oxides are versatile substances, often used in industrial processes that require a component to neutralize both acidic and basic contaminants. This dual property can also affect the material’s behavior under various environmental conditions.

Neutral Oxides

Neutral oxides stand out because they exhibit limited or no reactivity with acids or bases. This lack of significant interaction means they do not form salts or have a definable acidic or basic characteristic in common environments. Common examples - Carbon monoxide (CO) Understanding neutral oxides is essential in environmental chemistry, as their stability often translates to minimal impacts when released into the atmosphere. These oxides usually do not alter the pH of surroundings, making them chemically inert in typical reactions.