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Chapter 22: Problem 32

A friend tells you that the "neon" in neon signs is a compound of neon and aluminum. Can your friend be correct? Explain.

Short Answer

Expert verified
No, your friend is incorrect. Neon is a noble gas with a full octet of electrons, making it stable and not prone to forming compounds, while aluminum can form compounds by losing its 3 valence electrons. Since neon doesn't have any electrons available for bond formation, a compound of neon and aluminum is highly improbable.

Step by step solution

01

- Understanding Neon and Aluminum Properties

Neon (Ne) is a noble gas element with an atomic number of 10, while aluminum (Al) is a metal element with an atomic number of 13. We will examine their electron configurations to understand their bonding capabilities.
02

- Writing the Electron Configurations

To determine the electron configurations of the elements, we can use the periodic table as a guide. For neon (Ne), the electron configuration is: \(1s^2 2s^2 2p^6\) For aluminum (Al), the electron configuration is: \(1s^2 2s^2 2p^6 3s^2 3p^1\)
03

- Analyzing the Electron Configurations for Bond Formation

Now, we analyze the electron configurations to determine what type of bond, if any, can form between Neon and Aluminum. Neon has a completely filled outer shell (2s^2 2p^6) with 8 electrons, known as an octet. Noble gases usually don't form compounds due to their full octet, which indicates stability. Aluminum has 3 valence electrons in its outer shell (3s^2 3p^1). It can form compounds by losing its 3 valence electrons and forming an ionic bond with elements that can accept these electrons.
04

- Determine the Possibility of a Compound Formation

Since Neon has a stable electron configuration with a complete octet, it doesn't have a tendency to form compounds by sharing, losing, or accepting electrons. On the other hand, Aluminum can form a compound by losing its valence electrons to another element. Because Neon doesn't have any electrons available to form bonds, it is highly improbable that a compound of Neon and Aluminum can exist. Therefore, your friend's statement is incorrect.

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Most popular questions from this chapter

Explain the following observations: (a) The highest fluoride compound formed by nitrogen is \(\mathrm{NF}_{3}\), whereas phosphorus readily forms \(\mathrm{PF}_{5}\). (b) Although \(\mathrm{CO}\) is a well-known compound, SiO does not exist under ordinary conditions. (c) \(\mathrm{AsH}_{3}\) is a stronger reducing agent than \(\mathrm{NH}_{3} .\)

An aqueous solution of \(\mathrm{SO}_{2}\) reduces (a) aqueous \(\mathrm{KMnO}_{4}\) to \(\mathrm{MnSO}_{4}(a q),(\mathbf{b})\) acidic aqueous \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to aqueous \(\mathrm{Cr}^{3+},(\mathrm{c})\) aqueous \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}\) to mercury metal. Write balanced equations for these reactions.

You have two glass bottles, one containing oxygen and one filled with ozone. How could you determine which one is which? [Section 22.5\(]\)

Explain why \(\mathrm{SO}_{2}\) can be used as a reducing agent but \(\mathrm{SO}_{3}\) cannot.

Are the physical properties of \(\mathrm{H}_{2} \mathrm{O}\) different from \(\mathrm{D}_{2} \mathrm{O}\) ? Explain.
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