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Chapter 6: Problem 94

When sodium is treated with sufficient oxygen/air, the product obtained is:

Short Answer

Expert verified
Sodium reacts with oxygen to form sodium peroxide (Na鈧侽鈧�).

Step by step solution

01

Understanding the Reactants

We have sodium, a chemical element with the symbol Na, reacting with oxygen, which occurs in the air primarily as diatomic molecules (O鈧�). The key to this question is recognizing the type of compound sodium typically forms with oxygen.
02

Identify the Type of Compound Formed

When sodium reacts with oxygen, it forms an ionic compound. In this reaction, sodium donates electrons to oxygen, resulting in the formation of an oxide. Sodium can form different oxides depending on conditions, but in normal conditions, it forms sodium peroxide (Na鈧侽鈧�).
03

Write the Balanced Chemical Equation

The balanced chemical equation for the reaction of sodium with oxygen to primarily form sodium peroxide is:\[ 2 ext{Na} + ext{O}_2 ightarrow ext{Na}_2 ext{O}_2 \]This equation shows that two atoms of sodium react with one molecule of oxygen to form one molecule of sodium peroxide.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Reactions
The foundation of chemistry lies in understanding chemical reactions. These are processes where substances, known as reactants, transform into different substances called products. During a chemical reaction:
  • Bonds between atoms in the reactants are broken.
  • New bonds form to create the products.
  • Energy is often absorbed or released.
In the case of sodium reacting with oxygen, we start with elemental sodium (\(\text{Na}\)) and molecular oxygen (\(\text{O}_2\)). This type of reaction involves transfer of electrons, resulting in the formation of new compounds. Specifically, sodium transfers electrons to oxygen, completing the reaction. This is an example of an oxidation-reduction (redox) reaction where electron transfer plays a crucial role.
Sodium Peroxide Formation
Sodium peroxide (\(\text{Na}_2\text{O}_2\)) is the specific compound formed when sodium reacts with oxygen in normal conditions. Here's how this happens:
  • Sodium (\(\text{Na}\)) is a metal, known for easily losing electrons.
  • Oxygen (\(\text{O}_2\)) is a non-metal that tends to gain electrons.
  • When these react, sodium donates one electron to oxygen.
This donation establishes a stable ionic bond, forming sodium peroxide. Sodium peroxide is characterized by its ability to release oxygen, which makes it useful in situations where a controlled discharge of oxygen is needed, like in bleaching or portable oxygen generators.
Balanced Chemical Equations
Writing balanced chemical equations is essential in chemistry as they tell you the quantities and proportions of reactants and products involved in the reaction. Balancing a chemical equation:
  • Ensures that the same number of each type of atom appears on both sides of the equation.
  • Reflects the conservation of mass principle.
  • Makes sure the equation accurately represents the reaction.
For sodium and oxygen forming sodium peroxide, the balanced equation is:\[2\,\text{Na} + \text{O}_2 \rightarrow \text{Na}_2\text{O}_2\]This means two atoms of sodium combine with one molecule of oxygen to yield one formula unit of sodium peroxide. Balancing this equation ensures it obeys the law of conservation of mass, indicating that atoms are neither created nor destroyed during the reaction.

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Most popular questions from this chapter

In certain matters, lithium differs from other alkali metals, the main reason for this is: (a) small size of lithium atom and \(\mathrm{Li}^{+}\) (b) extremely high electropositivity of Li (c) greater hardness of \(\mathrm{Li}\) (d) hydration of \(\mathrm{Li}^{+}\) ion

\(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3} \cdot 5 \mathrm{H}_{2} \mathrm{O}\) is used in photography to: (a) reduce \(\mathrm{AgBr}\) to metallic \(\mathrm{Ag}\) (b) remove reduced \(\mathrm{Ag}\) (c) remove undecomposed \(\mathrm{AgBr}\) as a soluble complex \(\square\) (d) convert metallic Ag to silver salt \(\square\)

The chloride that can be extracted with ether is: (a) \(\mathrm{NaCl}\) \(\square\) (b) KCl (c) LiCl \(\square\) (d) \(\mathrm{RbCl}\)

What are the raw materials used in Solvay process? (a) \(\mathrm{NaCl}, \mathrm{NH}_{3}, \mathrm{CaCO}_{3} \quad \square\) (b) \(\mathrm{NaOH}, \mathrm{CO}_{2}\) (c) \(\mathrm{NaCl}, \mathrm{CO}_{2}\) (d) \(\mathrm{NaCl}, \mathrm{CaCO}_{3}, \mathrm{C}, \mathrm{H}_{2} \mathrm{SO}_{4}\)

Stable oxide is obtained by heating the carbonate of the element: (a) \(\mathrm{Li}\) (b) Na (c) \(\mathrm{K}\) (d) \(\mathrm{Rb}\)
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