Question

Give examples of two basic oxides. Write equations illustrating the formation of each oxide from its component elements. Write another chemical equation that illustrates the basic character of each oxide.

Short answer

Two basic oxides are \(\text{Na}_2\text{O}\) and \(\text{MgO}\). They form by reacting their elements with oxygen and display basic character by forming bases or reacting with acids.

Step-by-step solution

Identify Basic Oxides

Basic oxides are oxides that react with water to form bases or with acids to form salts and water. Two common examples of basic oxides are sodium oxide \(\text{Na}_2\text{O}\) and magnesium oxide \(\text{MgO}\).

Write Equation for Sodium Oxide Formation

Sodium oxide \(\text{Na}_2\text{O}\) is formed by reacting sodium with oxygen. The balanced chemical equation is:\[ 4\text{Na} + \text{O}_2 \rightarrow 2\text{Na}_2\text{O} \]

Write Equation for Magnesium Oxide Formation

Magnesium oxide \(\text{MgO}\) is formed by reacting magnesium with oxygen. The balanced chemical equation is:\[ 2\text{Mg} + \text{O}_2 \rightarrow 2\text{MgO} \]

Demonstrate Basic Character of Sodium Oxide

Sodium oxide \(\text{Na}_2\text{O}\) shows its basic character by reacting with water to form sodium hydroxide \(\text{NaOH}\), a strong base:\[ \text{Na}_2\text{O} + \text{H}_2\text{O} \rightarrow 2\text{NaOH} \]

Demonstrate Basic Character of Magnesium Oxide

Magnesium oxide \(\text{MgO}\) shows its basic character by reacting with hydrochloric acid \(\text{HCl}\) to form magnesium chloride \(\text{MgCl}_2\) and water:\[ \text{MgO} + 2\text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2\text{O} \]

Key concepts

Formation of Oxides

When we talk about the formation of oxides, we're exploring how elements react with oxygen. This interaction is a fundamental chemical process. Oxides are compounds that contain at least one oxygen atom paired with another element. In the world of chemistry, this often involves metals, and these compounds are known as metal oxides.

For example, both sodium and magnesium can react with oxygen to form their respective oxides. Sodium forms sodium oxide when it interacts with oxygen, represented by the balanced equation: - \(4\text{Na} + \text{O}_2 \rightarrow 2\text{Na}_2\text{O}\)This tells us that four atoms of sodium react with one molecule of oxygen gas to produce two units of sodium oxide.

Similarly, magnesium reacts with oxygen to form magnesium oxide:- \(2\text{Mg} + \text{O}_2 \rightarrow 2\text{MgO}\)In this equation, two magnesium atoms combine with one molecule of oxygen to produce two units of magnesium oxide.

These reactions occur easily when metals are heated in the presence of oxygen, showcasing the reactive nature of metals towards oxygen.

Chemical Equations

Chemical equations serve as the language of chemistry, depicting how substances change during a reaction. Each equation identifies the reactants on the left and the products on the right.

Balanced chemical equations are essential, meaning that the number of atoms for each element is the same on both sides of the equation. This adheres to the law of conservation of mass. For example, in the formation of sodium oxide:- \(4\text{Na} + \text{O}_2 \rightarrow 2\text{Na}_2\text{O}\)We see four sodium atoms and two oxygen atoms on each side of the equation. This balance ensures that the equation is correct and reflects what physically transpires in a reaction.

Similarly, for magnesium oxide formation:- \(2\text{Mg} + \text{O}_2 \rightarrow 2\text{MgO}\)Each side contains two magnesium and two oxygen atoms. Using balanced chemical equations helps chemists communicate complex reactions clearly and effectively.

In essence, writing and balancing chemical equations is crucial in understanding chemical changes and reactions.

Basic Character of Oxides

Oxides can possess different chemical natures, namely basic, acidic, amphoteric, or neutral. Basic oxides are typically metallic oxides that react with acids to form salt and water. They can also form hydroxides when they react with water.

Taking our previous example, sodium oxide exhibits basic characteristics because it reacts with water to form sodium hydroxide:- \(\text{Na}_2\text{O} + \text{H}_2\text{O} \rightarrow 2\text{NaOH}\)Sodium hydroxide is a strong base, which indicates the basic nature of sodium oxide.

Magnesium oxide, another basic oxide, demonstrates its character by reacting with hydrochloric acid to form magnesium chloride and water:- \(\text{MgO} + 2\text{HCl} \rightarrow \text{MgCl}_2 + \text{H}_2\text{O}\)This reaction highlights how magnesium oxide neutralizes an acid, resulting in a salt and water, classic behavior of a basic oxide.

Understanding the basic character of oxides helps in predicting their reactivity and applications, particularly in neutralizing acidic solutions.