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Chapter 22: Problem 42

Select the more acidic member of each of the following pairs: (a) \(\mathrm{Mn}_{2} \mathrm{O}_{7}\) and \(\mathrm{MnO}_{2}\), (b) \(\mathrm{SnO}\) and \(\mathrm{SnO}_{2}\), (c) \(\mathrm{SO}_{2}\) and \(\mathrm{SO}_{3}\), (d) \(\mathrm{SiO}_{2}\) and \(\mathrm{SO}_{2}\), (e) \(\mathrm{Ga}_{2} \mathrm{O}_{3}\) and \(\mathrm{In}_{2} \mathrm{O}_{3},\) (f) \(\mathrm{SO}_{2}\) and \(\mathrm{SeO}_{2}\).

Short Answer

Expert verified
The more acidic members of the given pairs are: (a) \(\mathrm{Mn}_{2} \mathrm{O}_{7}\), (b) \(\mathrm{SnO}_{2}\), (c) \(\mathrm{SO}_{3}\), (d) \(\mathrm{SO}_{2}\), (e) \(\mathrm{Ga}_{2} \mathrm{O}_{3}\), and (f) \(\mathrm{SO}_{2}\).

Step by step solution

01

Pair (a): \(\mathrm{Mn}_{2} \mathrm{O}_{7}\) and \(\mathrm{MnO}_{2}\)

Manganese heptoxide (\(\mathrm{Mn}_{2} \mathrm{O}_{7}\)) is a compound in which manganese has an oxidation state of +7, while manganese dioxide (\(\mathrm{MnO}_{2}\)) has manganese in the +4 oxidation state. Higher oxidation states generally result in a more acidic compound because the central atom is more electronegative and can stabilize the conjugate base better. Therefore, \(\mathrm{Mn}_{2} \mathrm{O}_{7}\) is the more acidic member of this pair.
02

Pair (b): \(\mathrm{SnO}\) and \(\mathrm{SnO}_{2}\)

For tin monoxide (\(\mathrm{SnO}\)), tin has an oxidation state of +2, while for tin dioxide (\(\mathrm{SnO}_{2}\)), the oxidation state is +4. As discussed in the previous pair, compounds with higher oxidation states are generally more acidic. Therefore, \(\mathrm{SnO}_{2}\) is the more acidic member of this pair.
03

Pair (c): \(\mathrm{SO}_{2}\) and \(\mathrm{SO}_{3}\)

Sulfur dioxide (\(\mathrm{SO}_{2}\)) has sulfur in the +4 oxidation state, while sulfur trioxide (\(\mathrm{SO}_{3}\)) has sulfur in the +6 oxidation state. Due to the higher electronegativity and oxidation state in \(\mathrm{SO}_{3}\), it is more acidic than \(\mathrm{SO}_{2}\).
04

Pair (d): \(\mathrm{SiO}_{2}\) and \(\mathrm{SO}_{2}\)

Silicon dioxide (\(\mathrm{SiO}_{2}\)) has silicon in the +4 oxidation state, while sulfur dioxide (\(\mathrm{SO}_{2}\)) has sulfur in the +4 oxidation state. Though both central atoms have the same oxidation state, sulfur is more electronegative than silicon. Thus, \(\mathrm{SO}_{2}\) is more acidic than \(\mathrm{SiO}_{2}\).
05

Pair (e): \(\mathrm{Ga}_{2} \mathrm{O}_{3}\) and \(\mathrm{In}_{2} \mathrm{O}_{3}\)

Gallium oxide (\(\mathrm{Ga}_{2} \mathrm{O}_{3}\)) has gallium in the +3 oxidation state, as does indium oxide (\(\mathrm{In}_{2} \mathrm{O}_{3}\)) for indium. They are in the same group in the periodic table, so we must compare their electronegativities. Gallium is more electronegative than indium, so \(\mathrm{Ga}_{2} \mathrm{O}_{3}\) is the more acidic member of this pair.
06

Pair (f): \(\mathrm{SO}_{2}\) and \(\mathrm{SeO}_{2}\)

Sulfur dioxide (\(\mathrm{SO}_{2}\)) has sulfur in the +4 oxidation state, and selenium dioxide (\(\mathrm{SeO}_{2}\)) has selenium in the +4 oxidation state. Both are in the same group in the periodic table, so we must compare their electronegativities. Sulfur is more electronegative than selenium, so \(\mathrm{SO}_{2}\) is the more acidic member of this pair.

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Most popular questions from this chapter

Write the Lewis structure for each of the following species, describe its geometry, and indicate the oxidation state of the (a) \(\mathrm{NH}_{4}^{+},(\mathbf{b}) \mathrm{NO}_{2}^{-}\), nitrogen: (c) \(\mathrm{N}_{2} \mathrm{O},(\mathrm{d}) \mathrm{NO}_{2}\)

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

Give the chemical formula for (a) carbonic acid, (b) sodium cyanide, (c) potassium hydrogen carbonate, (d) acetylene, (e) iron pentacarbonyl.

Why does xenon form stable compounds with fluorine, whereas argon does not?

One method proposed for removing \(\mathrm{SO}_{2}\) from the flue gases of power plants involves reaction with aqueous \(\mathrm{H}_{2} \mathrm{~S}\). Elemental sulfur is the product. (a) Write a balanced chemical equation for the reaction. (b) What volume of \(\mathrm{H}_{2} \mathrm{~S}\) at \(27^{\circ} \mathrm{C}\) and 760 torr would be required to remove the \(\mathrm{SO}_{2}\) formed by burning 2.0 tons of coal containing \(3.5 \% \mathrm{~S}\) by mass? (c) What mass of elemental sulfur is produced? Assume that all reactions are \(100 \%\) efficient.
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