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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
Your friend's statement is incorrect. The "neon" in neon signs is not a compound of neon and aluminum because neon is a noble gas with a full valence electron shell, making it unreactive and unlikely to form compounds with other elements, such as aluminum.

Step by step solution

01

Understand Neon and Compounds

First, let's understand the nature of neon. Neon is a noble gas, which means it has a full electron shell and rarely forms chemical bonds. Noble gases are very stable and unreactive due to their full electron shell, making it difficult for them to form compounds with other elements. Now let's understand compounds. A compound is a substance that forms when two or more elements chemically combine, resulting in a new substance with different properties from the original elements. For a compound to form, there should be a chemical reaction between the elements.
02

Analyze the possibility of neon forming a compound with aluminum

Since neon is a noble gas and has a full valence shell, it tends not to participate in chemical reactions to form compounds. Aluminum, on the other hand, is a reactive metal with a partially-filled electron valence shell that readily engages in chemical reactions. Considering the nature of neon and aluminum, it is unlikely that they would form a compound, as neon's unreactive nature would not allow it to form a chemical bond with aluminum.
03

Conclusion

Based on our understanding of neon and its unreactive nature, we can conclude that your friend's statement is incorrect. The "neon" in neon signs is not a compound of neon and aluminum, as neon is a noble gas that rarely forms compounds with other elements due to its full valence electron shell.

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Most popular questions from this chapter

(a) What is the characteristic geometry about silicon in all silicate minerals? (b) Metasilicic acid has the empirical formula \(\mathrm{H}_{2} \mathrm{SiO}_{3}\). Which of the structures shown in Figure \(22.34\) would you expect metasilicic acid to have? 22.76 Speculate as to why carbon forms carbonate rather than silicate analogs.

Ultrapure germanium, like silicon, is used in semiconductors. Germanium of "ordinary" purity is prepared by the high-temperature reduction of \(\mathrm{GeO}_{2}\) with carbon. The Ge is converted to \(\mathrm{GeCl}_{4}\) by treatment with \(\mathrm{Cl}_{2}\) and then purified by distillation; \(\mathrm{GeCl}_{4}\) is then hydrolyzed in water to \(\mathrm{GeO}_{2}\) and reduced to the elemental form with \(\mathrm{H}_{2}\). The element is then zone refined. Write a balanced chemical equation for each of the chemical transformations in the course of forming ultrapure Ge from \(\mathrm{GeO}_{2}\).

Write balanced equations for each of the following reactions. (a) When mercury(II) oxide is heated, it decomposes to form \(\mathrm{O}_{2}\) and mercury metal. (b) When copper(II) nitrate is heated strongly, it decomposes to form copper(II) oxide, nitrogen dioxide, and oxygen. (c) Lead(II) sulfide, \(\mathrm{PbS}(s)\), reacts with ozone to form \(\mathrm{PbSO}_{4}(s)\) and \(\mathrm{O}_{2}(g)\). (d) When heated in air, \(\mathrm{ZnS}(s)\) is converted to \(\mathrm{ZnO}\). (e) Potassium peroxide reacts with \(\mathrm{CO}_{2}(g)\) to give potassium carbonate and \(\mathrm{O}_{2}\) (f) Oxygen is converted to ozone in the upper atmosphere.

Complete and balance the following equations: (a) \(\mathrm{NaOCH}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{CuO}(s)+\mathrm{HNO}_{3}(a q) \longrightarrow\) (c) \(\mathrm{WO}_{3}(s)+\mathrm{H}_{2}(g) \stackrel{\Delta}{\longrightarrow}\) (d) \(\mathrm{NH}_{2} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow\) (c) \(\mathrm{Al}_{1} \mathrm{C}_{1}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\)

Chemists tried for a long time to make molecular compounds containing silicon- silicon double bonds, they finally succeeded in 1981 . The trick is having large, bulky R groups on the silicon atoms to make \(\mathrm{R}_{2} \mathrm{Si}=\mathrm{SiR}_{2}\) compounds. What experiments could you do to prove that a new compound has a silicon-silicon double bond rather than a silicon-silicon single bond?
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