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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
Sc2O3 is an amphoteric metal oxide, meaning it can react with both acidic and basic solutions. The balanced chemical equations are: Reaction with an acid (H+ ions): \( Sc_2O_3 + 6H^+ \rightarrow 2Sc^{3+} + 3H_2O \) Reaction with a base (OH- ions): \( Sc_2O_3 + 6OH^- \rightarrow 2Sc(OH)_6^{3-} \)

Step by step solution

01

Analyze the given compound Sc2O3

Sc2O3 is a metal oxide, which means it is composed of a metal (Sc) and oxygen (O). Metal oxides tend to be either basic or amphoteric, meaning they can react with either acids or bases.
02

Predict if Sc2O3 is basic or amphoteric

Sc2O3 is composed of scandium, which is a metal from Group 3 of the periodic table. Group 3 metal oxides typically display amphoteric behavior, meaning they can react with both acidic and basic solutions. We can therefore predict that Sc2O3 will react with acidic and basic solutions.
03

Write balanced chemical equations for reactions with acids and bases

As Sc2O3 is amphoteric, it will react with both acidic and basic solutions. Let's write balanced chemical equations for both reactions. Reaction with an acid (H+ ions): \( Sc_2O_3 + 6H^+ \rightarrow 2Sc^{3+} + 3H_2O \) Reaction with a base (OH- ions): \( Sc_2O_3 + 6OH^- \rightarrow 2Sc(OH)_6^{3-} \) We have now written balanced chemical equations for the reaction of Sc2O3 with acidic and basic solutions. Sc2O3 will react with both acidic and basic solutions since it is an amphoteric metal oxide.

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Most popular questions from this chapter

Write the electron configurations for the following ions, and determine which have noble-gas configurations: (a) \(\mathrm{Ru}^{3+}\), (b) \(\mathrm{As}^{3-}\), (c) \(\mathrm{Y}^{3+}\), (d) \(\mathrm{Pd}^{2+}\), (e) \(\mathrm{Pb}^{2+}\), (f) \(\mathrm{Au}^{3+}\).

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Chlorine reacts with water. (b) Barium metal is heated in an atmosphere of hydrogen gas. (c) Lithium reacts with sulfur. (d) Fluorine reacts with magnesium metal.

Arrange each of the following sets of atoms and ions, in order of increasing size: (a) \(\mathrm{Se}^{2-}, \mathrm{Te}^{2-}, \mathrm{Se} ;\) (b) \(\mathrm{Co}^{3+}, \mathrm{Fe}^{2+}, \mathrm{Fe}^{3+}\); (c) \(\mathrm{Ca}^{2 \mathrm{Ti}^{4+}}, \mathrm{Sc}^{3+}\); (d) \(\mathrm{Be}^{2+}, \mathrm{Na}^{+}, \mathrm{Ne}\).

Mercury in the environment can exist in oxidation states \(0,+1\), and \(+2\). One major question in environmental chemistry research is how to best measure the oxidation state of mercury in natural systems; this is made more complicated by the fact that mercury can be reduced or oxidized on surfaces differently than it would be if it were free in solution. XPS, X-ray photoelectron spectroscopy, is a technique related to PES (see Exercise 7.111), but instead of using ultraviolet light to eject valence electrons, \(\mathrm{X}\) rays are used to eject core electrons. The energies of the core electrons are different for different oxidation states of the element. In one set of experiments, researchers examined mercury contamination of minerals in water. They measured the XPS signals that corresponded to electrons ejected from mercury's \(4 f\) orbitals at \(105 \mathrm{eV}\), from an X-ray source that provided \(1253.6 \mathrm{eV}\) of energy. The oxygen on the mineral surface gave emitted electron energies at \(531 \mathrm{eV}\), corresponding to the \(1 s\) orbital of oxygen. Overall the researchers concluded that oxidation states were \(+2\) for \(\mathrm{Hg}\) and \(-2\) for \(\mathrm{O}\). (a) Calculate the wavelength of the \(\mathrm{X}\) rays used in this experiment. (b) Compare the energies of the \(4 f\) electrons in mercury and the \(1 s\) electrons in oxygen from these data to the first ionization energies of mercury and oxygen from the data in this chapter. (c) Write out the ground-state electron configurations for \(\mathrm{Hg}^{2+}\) and \(\mathrm{O}^{2-}\); which electrons are the valence electrons in each case? (d) Use Slater's rules to estimate \(Z_{\text {eff }}\) for the \(4 f\) and valence electrons of \(\mathrm{Hg}^{2+}\) and \(\mathrm{O}^{2-}\); assume for this purpose that all the inner electrons with \((n-3)\) or less screen a full \(+1\).

Write equations that show the processes that describe the first, second, and third ionization energies of an aluminum atom. Which process would require the least amount of energy?
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