Chapter 7: Problem 79
Write balanced equations for the reactions between each of the following oxides and water: (a) \(\mathrm{Li}_{2} \mathrm{O}\) (b) \(\mathrm{CaO}\) (c) \(\mathrm{SO}_{3}\)
Short Answer
Expert verified
(a) \(\text{Li}_2\text{O} + \text{H}_2\text{O} \rightarrow 2\text{LiOH}\); (b) \(\text{CaO} + \text{H}_2\text{O} \rightarrow \text{Ca(OH)}_2\); (c) \(\text{SO}_3 + \text{H}_2\text{O} \rightarrow \text{H}_2\text{SO}_4\).
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Basic Oxides
Basic oxides are typically formed when metals react with oxygen. These oxides, such as \( \text{Li}_2 \text{O} \) (lithium oxide) and \( \text{CaO} \) (calcium oxide), are generally ionic in nature. A characteristic of basic oxides is their ability to react with water to form hydroxides, which are basic compounds.
If a basic oxide like lithium oxide comes into contact with water, it undergoes a chemical reaction resulting in the formation of a metal hydroxide. This showcases the typical behavior of metals: they lose electrons easily. Basic oxides tend to have high melting points, indicating a strong attraction between their ionic particles.
To sum up, basic oxides form from metals, react with water to yield hydroxides, and are known for their ionic bonds and high melting points.
If a basic oxide like lithium oxide comes into contact with water, it undergoes a chemical reaction resulting in the formation of a metal hydroxide. This showcases the typical behavior of metals: they lose electrons easily. Basic oxides tend to have high melting points, indicating a strong attraction between their ionic particles.
To sum up, basic oxides form from metals, react with water to yield hydroxides, and are known for their ionic bonds and high melting points.
Acidic Oxides
Acidic oxides are primarily formed when nonmetals react with oxygen. These substances, such as \( \text{SO}_3 \) (sulfur trioxide), are different from basic oxides because they are covalent in nature. When acidic oxides react with water, they form acids.
For instance, when sulfur trioxide interacts with water, it forms sulfuric acid, a well-known acid in chemistry. The reaction of acidic oxides with water highlights their tendency to attract electrons, characteristic of nonmetals. Unlike basic oxides, acidic oxides often have lower melting and boiling points due to the weaker forces between their covalent molecules.
In brief, acidic oxides come from nonmetals, transform into acids when water is added, and possess covalent bonds.
For instance, when sulfur trioxide interacts with water, it forms sulfuric acid, a well-known acid in chemistry. The reaction of acidic oxides with water highlights their tendency to attract electrons, characteristic of nonmetals. Unlike basic oxides, acidic oxides often have lower melting and boiling points due to the weaker forces between their covalent molecules.
In brief, acidic oxides come from nonmetals, transform into acids when water is added, and possess covalent bonds.
Reaction of Oxides with Water
When oxides react with water, the process greatly depends on whether the oxide is basic or acidic.
The reaction with basic oxides results in the formation of hydroxides, which are basic solutions. For example, adding water to \( \text{CaO} \) yields calcium hydroxide. On the flip side, the reaction of acidic oxides, like \( \text{SO}_3 \), with water forms acids. In this case, sulfur trioxide interacting with water produces sulfuric acid.
These reactions are crucial in many environmental and industrial processes. For example, the reaction of sulfur trioxide with water is part of the formation of acid rain.
Essentially, the nature of the oxide dictates whether a base or acid is formed in its reaction with water.
The reaction with basic oxides results in the formation of hydroxides, which are basic solutions. For example, adding water to \( \text{CaO} \) yields calcium hydroxide. On the flip side, the reaction of acidic oxides, like \( \text{SO}_3 \), with water forms acids. In this case, sulfur trioxide interacting with water produces sulfuric acid.
- The general equation for basic oxides: \( \text{Metal oxide + Water} \rightarrow \text{Metal hydroxide} \)
- The general equation for acidic oxides: \( \text{Non-metal oxide + Water} \rightarrow \text{Acid} \)
These reactions are crucial in many environmental and industrial processes. For example, the reaction of sulfur trioxide with water is part of the formation of acid rain.
Essentially, the nature of the oxide dictates whether a base or acid is formed in its reaction with water.
Formation of Hydroxides and Acids
Hydroxides and acids are formed when their respective oxides react with water. The outcome of this reaction highlights the inherent properties of the elements forming the oxides.
For basic oxides, the reaction with water produces hydroxides. Take \( \text{Li}_2 \text{O} \), which reacts with water to form lithium hydroxide. Hydroxides are compounds that contain the hydroxide ion \( \text{OH}^- \) and are typically basic in nature. They play a crucial role in many chemical reactions, including neutralization reactions.
In contrast, acidic oxides such as \( \text{SO}_3 \) form acids when they react with water. When \( \text{SO}_3 \) combines with water, the result is sulfuric acid, a vital substance in industry and chemistry. These acids contain hydrogen ions \( \text{H}^+ \), which is why they are acids.
Understanding these reactions is key to grasping how substances can change their chemical properties through interactions with water, leading to the formation of bases or acids.
For basic oxides, the reaction with water produces hydroxides. Take \( \text{Li}_2 \text{O} \), which reacts with water to form lithium hydroxide. Hydroxides are compounds that contain the hydroxide ion \( \text{OH}^- \) and are typically basic in nature. They play a crucial role in many chemical reactions, including neutralization reactions.
In contrast, acidic oxides such as \( \text{SO}_3 \) form acids when they react with water. When \( \text{SO}_3 \) combines with water, the result is sulfuric acid, a vital substance in industry and chemistry. These acids contain hydrogen ions \( \text{H}^+ \), which is why they are acids.
Understanding these reactions is key to grasping how substances can change their chemical properties through interactions with water, leading to the formation of bases or acids.
