Problem 62 - Chemistry The Central Science In Si Units

Question

Arrange the following oxides in order of increasing acidity: \(\mathrm{K}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{ZnO}, \mathrm{H}_{2} \mathrm{O}, \mathrm{CO}_{2}, \mathrm{SO}_{2}\).

Step-by-Step Solution

Answer

The order of increasing acidity is: \(\mathrm{K}_2 \mathrm{O}, \mathrm{BaO}, \mathrm{ZnO}, \mathrm{H}_2 \mathrm{O}, \mathrm{CO}_2, \mathrm{SO}_2\).

Step 1: Understanding Oxide Acid-Base Behavior

First, recognize that metal oxides are typically basic, whereas non-metal oxides are generally acidic. This fundamental understanding will help us categorize each given oxide into basic, amphoteric, or acidic.

Step 2: Identify Metal and Non-Metal Oxides

The metal oxides in the list are: - \(\mathrm{K}_2 \mathrm{O}\) (Potassium Oxide)- \(\mathrm{BaO}\) (Barium Oxide)- \(\mathrm{ZnO}\) (Zinc Oxide). The non-metal oxides include: - \(\mathrm{H}_2 \mathrm{O}\) (Water)- \(\mathrm{CO}_2\) (Carbon Dioxide)- \(\mathrm{SO}_2\) (Sulfur Dioxide).

Step 3: Classify Oxides

Classify the oxides based on their properties: 1. Basic Oxides: \(\mathrm{K}_2 \mathrm{O}\) and \(\mathrm{BaO}\).2. Amphoteric Oxide: \(\mathrm{ZnO}\).3. Neutral Oxide: \(\mathrm{H}_2 \mathrm{O}\).4. Acidic Oxides: \(\mathrm{CO}_2\) and \(\mathrm{SO}_2\).

Step 4: Rank Oxides by Increasing Acidity

Arrange the oxides from the least to the most acidic:1. \(\mathrm{K}_2 \mathrm{O}\) and \(\mathrm{BaO}\) (basic, least acidic)2. \(\mathrm{ZnO}\) (amphoteric)3. \(\mathrm{H}_2 \mathrm{O}\) (neutral)4. \(\mathrm{CO}_2\)5. \(\mathrm{SO}_2\) (most acidic).

Key Concepts

Metal Oxides

Metal oxides are compounds formed between metals and oxygen. These oxides are generally basic in nature. This means they have a tendency to accept protons from water when dissolved, forming hydroxide ions. For example, potassium oxide (\(\mathrm{K}_2 \mathrm{O}\)) and barium oxide (\(\mathrm{BaO}\)) can combine with water to form basic solutions.

• Pounds like \(\mathrm{K}_2 \mathrm{O}\): Reacts with water to form potassium hydroxide, \(\mathrm{KOH}\).
• \(\mathrm{BaO}\): Reacts with water to form barium hydroxide, \(\mathrm{Ba(OH)_2}\).

These reactions show that metal oxides readily form bases by accepting hydrogen ions. They are typically found in the left and middle of the periodic table, where metallic elements are positioned.

Non-Metal Oxides

In contrast to metal oxides, non-metal oxides usually exhibit acidic characteristics. These are compounds formed between non-metals and oxygen, which tend to donate protons and form acids in water. For example, carbon dioxide (\(\mathrm{CO}_2\)) and sulfur dioxide (\(\mathrm{SO}_2\)) are well-known non-metal oxides. When dissolved in water, these oxides can form acidic solutions such as carbonic acid and sulfurous acid respectively.

• When \(\mathrm{CO}_2\) is in water, it forms carbonic acid (\(\mathrm{H}_2\mathrm{CO}_3\)).
• \(\mathrm{SO}_2\) in water results in sulfurous acid (\(\mathrm{H}_2\mathrm{SO}_3\)).

These reactions illustrate the acidic behavior of non-metal oxides, making them key contributors to phenomena like acid rain when released into the atmosphere.

Classification of Oxides

Oxides can be neatly classified based on their chemical behavior in different categories: basic, acidic, amphoteric, and neutral. This classification helps us understand their properties and potential reactions.

• **Basic Oxides:** Formed by metals, like \(\mathrm{K}_2 \mathrm{O}\) and \(\mathrm{BaO}\), reacting with water to yield bases.
• **Acidic Oxides:** Derived mainly from non-metals, like \(\mathrm{CO}_2\) and \(\mathrm{SO}_2\), that produce acids in water.
• **Amphoteric Oxides:** Have properties of both acidic and basic oxides. Zinc oxide (\(\mathrm{ZnO}\)) is a great example, capable of reacting with both acids and bases.
• **Neutral Oxides:** Species like water (\(\mathrm{H}_2 \mathrm{O}\)) are considered neutral; they don't exhibit prominent acidic or basic properties.

Understanding these categories helps us predict their behavior in chemical reactions and their role in various natural and industrial processes.