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Chapter 7: Problem 60

Some metal oxides, such as \(\mathrm{Sc}_{2} \mathrm{O}_{3},\) do not react with pure water, but they do react when the solution becomes either acidic or basic. Do you expect \(\mathrm{Sc}_{2} \mathrm{O}_{3}\) to react when the solution becomes acidic or when it becomes basic? Write a balanced chemical equation to support your answer.

Short Answer

Expert verified
We expect \(\mathrm{Sc}_{2} \mathrm{O}_{3}\) to react in an acidic environment since it's a basic oxide. The balanced chemical equation for this reaction is: \[\mathrm{Sc}_{2} \mathrm{O}_{3} + 6 \mathrm{H}^{+} \rightarrow 2 \mathrm{Sc}^{3+} + 3 \mathrm{H}_{2} \mathrm{O}\].

Step by step solution

01

Identify the nature of the metal oxide

First, we need to determine whether the given metal oxide, \(\mathrm{Sc}_{2} \mathrm{O}_{3}\), is an acidic oxide or a basic oxide. This can be done by analyzing the position of the metallic element (Scandium, Sc) in the periodic table. Scandium is a metal from Group 3 and thus expected to form basic oxide.
02

Predict the reaction environment

Since \(\mathrm{Sc}_{2} \mathrm{O}_{3}\) is a basic oxide, it will react in an acidic environment. In an acidic environment, there will be a higher concentration of H+ ions, which will allow the basic oxide to react and neutralize the excess H+.
03

Write a balanced chemical equation

Now, let's write a balanced chemical equation for the reaction between the basic oxide \(\mathrm{Sc}_{2} \mathrm{O}_{3}\) and an acid, represented here as \(\mathrm{H}^{+}\). Since \(\mathrm{Sc}_{2} \mathrm{O}_{3}\) is a basic oxide, it would react with 6 H+ ions to form 2 Scandium ions and 3 Water molecules: \[\mathrm{Sc}_{2} \mathrm{O}_{3} + 6 \mathrm{H}^{+} \rightarrow 2 \mathrm{Sc}^{3+} + 3 \mathrm{H}_{2} \mathrm{O}\] In this balanced chemical equation, the basic oxide \(\mathrm{Sc}_{2} \mathrm{O}_{3}\) reacts with H+ ions from the acidic environment to produce Scandium ions and water molecules. This supports our prediction that \(\mathrm{Sc}_{2} \mathrm{O}_{3}\) will react in an acidic environment.

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Most popular questions from this chapter

It is possible to define metallic character as we do in this book and base it on the reactivity of the element and the ease with which it loses electrons. Alternatively, one could measurehow well electricity is conducted by each of the elements to determine how "metallic" the elements are. On the basis of conductivity, there is not much of a trend in the periodic table: silver is the most conductive metal, and manganese the least. Look up the first ionization energies of silver and manganese; which of these two elements would you call more metallic based on the way we define it in this book?

Potassium superoxide, \(\mathrm{KO}_{2},\) is often used in oxygen masks (such as those used by firefighters) because \(\mathrm{KO}_{2}\) reacts with \(\mathrm{CO}_{2}\) to release molecular oxygen. Experiments indicate that 2 \(\mathrm{mol}\) of \(\mathrm{KO}_{2}(s)\) react with each mole of= \(\mathrm{CO}_{2}(g) .\) (a) The products of the reaction are \(\mathrm{K}_{2} \mathrm{CO}_{3}(s)\) and \(\mathrm{O}_{2}(g) .\) Write a balanced equation for the reaction between \(\mathrm{KO}_{2}(s)\) and \(\mathrm{CO}_{2}(g) .(\mathbf{b})\) Indicate the oxidation number for each atom involved in the reaction in part (a). What elements are being oxidized and reduced? (c) What mass of \(\mathrm{KO}_{2}(s)\) is needed to consume 18.0 \(\mathrm{g} \mathrm{CO}_{2}(g) ?\) What mass of \(\mathrm{O}_{2}(g)\) is produced during this reaction?

Write equations that show the process for (a) the first two ionization energies of lead and (b) the fourth ionization energy of zirconium.

We will see in Chapter 12 that semiconductors are materials that conduct electricity better than nonmetals but not as well as metals. The only two elements in the periodic table that are technologically useful semiconductors are silicon and germanium. Integrated circuits in computer chips today are based on silicon. Compound semiconductors are also used in the electronics industry. Examples are gallium arsenide, GaAs; gallium phosphide, GaP; cadmium sulfide, CdS; and cadmium selenide, CdSe. (a) What is the relationship between the compound semiconductors’ compositions and the positions of their elements on the periodic table relative to Si and Ge? (b) Workers in the semiconductor industry refer to "II–VI" and "III–V" materials, using Roman numerals. Can you identify which compound semiconductors are II–VI and which are III–V? (c) Suggest other compositions of compound semiconductors based on the positions of their elements in the periodic table.

What is the relationship between the ionization energy of an anion with a \(1-\) charge such as \(F^{-}\) and the electron affinity of the neutral atom, \(\mathrm{F}\) ?
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