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Chapter 22: Problem 44

Write the chemical formula for each of the following compounds, and indicate the oxidation state of the group \(6 \mathrm{~A}\) element in each: (a) sulfur tetrachloride, (b) selenium trioxide, (c) sodium thiosulfate, (d) hydrogen sulfide, (e) sulfuric acid, \((\mathbf{f})\) sulfur dioxide, \((\mathrm{g})\) mercury telluride.

Short Answer

Expert verified
(a) Sulfur tetrachloride: \(\text{S}\text{Cl}_4\), oxidation state of sulfur is +4. (b) Selenium trioxide: \(\text{Se}{\text{O}}_3\), oxidation state of selenium is +6. (c) Sodium thiosulfate: \(\text{Na}_2\text{S}_2\text{O}_3\), oxidation state of sulfur is +2. (d) Hydrogen sulfide: \(\text{H}_2\text{S}\), oxidation state of sulfur is -2. (e) Sulfuric acid: \(\text{H}_2\text{SO}_4\), oxidation state of sulfur is +6. (f) Sulfur dioxide: \(\text{SO}_2\), oxidation state of sulfur is +4. (g) Mercury telluride: \(\text{HgTe}\), oxidation state of tellurium is -2.

Step by step solution

01

(a) Sulfur tetrachloride

Sulfur tetrachloride contains one sulfur atom (S) and four chlorine atoms (Cl). The chemical formula for this compound is \(\text{S}\text{Cl}_4\). Now, to find the oxidation state of sulfur: Each chlorine atom has an oxidation state of -1, so four chlorine atoms will have a total oxidation state of -4. As the sulfur atom needs to balance the oxidation states, it will have an oxidation state of +4. Hence, the oxidation state of sulfur in \(\text{S}\text{Cl}_4\) is +4.
02

(b) Selenium trioxide

Selenium trioxide contains one selenium atom (Se) and three oxygen atoms (O). The chemical formula for this compound is \(\text{Se}{\text{O}}_3\). Now, to find the oxidation state of selenium: Each oxygen atom has an oxidation state of -2, so three oxygen atoms will have a total oxidation state of -6. As the selenium atom needs to balance the oxidation state, it will have an oxidation state of +6. Hence, the oxidation state of selenium in \(\text{Se}{\text{O}}_3\) is +6.
03

(c) Sodium thiosulfate

Sodium thiosulfate contains two sodium atoms (Na), one sulfur atom (S), and three oxygen atoms (O). The chemical formula for this compound is \(\text{Na}_2\text{S}_2\text{O}_3\). Now, to find the oxidation state of sulfur: Each sodium atom has an oxidation state of +1, so two sodium atoms will have a total oxidation state of +2. Each oxygen atom has an oxidation state of -2, so three oxygen atoms will have a total oxidation state of -6. As the total oxidation state for sulfur will balance that of sodium and oxygen, the oxidation state of two sulfur atoms will be +4. Thus, for a single sulfur atom, the oxidation state in sodium thiosulfate is +2.
04

(d) Hydrogen sulfide

Hydrogen sulfide contains two hydrogen atoms (H) and one sulfur atom (S). The chemical formula for this compound is \(\text{H}_2\text{S}\). Now, to find the oxidation state of sulfur: Each hydrogen atom has an oxidation state of +1, so two hydrogen atoms will have a total oxidation state of +2. As the sulfur atom needs to balance the oxidation state, it will have an oxidation state of -2. Hence, the oxidation state of sulfur in \(\text{H}_2\text{S}\) is -2.
05

(e) Sulfuric acid

Sulfuric acid contains two hydrogen atoms (H), one sulfur atom (S), and four oxygen atoms (O). The chemical formula for this compound is \(\text{H}_2\text{SO}_4\). Now, to find the oxidation state of sulfur: Each hydrogen atom has an oxidation state of +1, so two hydrogen atoms will have a total oxidation state of +2. Each oxygen atom has an oxidation state of -2, so four oxygen atoms will have a total oxidation state of -8. As the sulfur atom needs to balance the oxidation state, it will have an oxidation state of +6. Hence, the oxidation state of sulfur in \(\text{H}_2\text{SO}_4\) is +6.
06

(f) Sulfur dioxide

Sulfur dioxide contains one sulfur atom (S) and two oxygen atoms (O). The chemical formula for this compound is \(\text{SO}_2\). Now, to find the oxidation state of sulfur: Each oxygen atom has an oxidation state of -2, so two oxygen atoms will have a total oxidation state of -4. As the sulfur atom needs to balance the oxidation state, it will have an oxidation state of +4. Hence, the oxidation state of sulfur in \(\text{SO}_2\) is +4.
07

(g) Mercury telluride

Mercury telluride contains one mercury atom (Hg) and one tellurium atom (Te). The chemical formula for this compound is \(\text{HgTe}\). Now, to find the oxidation state of tellurium: Mercury has an oxidation state of +2. As the tellurium atom needs to balance the oxidation state, it will have an oxidation state of -2. Hence, the oxidation state of tellurium in \(\text{HgTe}\) is -2.

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Most popular questions from this chapter

What is the anhydride for each of the following acids: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (b) \(\mathrm{HClO}_{3}\) (c) \(\mathrm{HNO}_{2}\), (d) \(\mathrm{H}_{2} \mathrm{CO}_{3},\) (e) \(\mathrm{H}_{3} \mathrm{PO}_{4} ?\)

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.

(a) How does the structure of diborane \(\left(\mathrm{B}_{2} \mathrm{H}_{6}\right)\) differ from that of ethane \(\left(\mathrm{C}_{2} \mathrm{H}_{6}\right) ?\) (b) Explain why diborane adopts the geometry that it does. (c) What is the significance of the statement that the hydrogen atoms in diborane are described as "hydridic'?

(a) Draw the Lewis structures for at least four species that have the general formula $$ [: X=Y:]^{n} $$ where \(\mathrm{X}\) and \(\mathrm{Y}\) may be the same or different, and \(n\) may have a value from +1 to -2 . (b) Which of the compounds is likely to be the strongest Bronsted base? Explain. [Sections \(22.1,22.7,\) and 22.9\(]\)

Write a balanced net ionic equation for each of the following reactions: (a) Dilute nitric acid reacts with zinc metal with formation of nitrous oxide. (b) Concentrated nitric acid reacts with sulfur with formation of nitrogen dioxide. (c) Concentrated nitric acid oxidizes sulfur dioxide with formation of nitric oxide. (d) Hydrazine is burned in excess fluorine gas, forming \(\mathrm{NF}_{3}\). (e) Hydrazine reduces \(\mathrm{CrO}_{4}^{2-}\) to \(\mathrm{Cr}(\mathrm{OH})_{4}^{-}\) in base (hydrazine is oxidized to \(\mathrm{N}_{2}\) ).
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