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Chapter 22: Problem 42

Write the chemical formula for each of the following com- pounds, 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, ( ( ) sulfur dioxide, (g) mercury telluride.

Short Answer

Expert verified
The chemical formulas and oxidation states for the given compounds are as follows: a) Sulfur Tetrachloride: \(S\mathrm{Cl_4}\), oxidation state of sulfur is +4. b) Selenium Trioxide: \(\mathrm{SeO_3}\), oxidation state of selenium is +6. c) Sodium Thiosulfate: \(\mathrm{Na_2S_2O_3}\), average oxidation state of sulfur is +2. d) Hydrogen Sulfide: \(\mathrm{H_2S}\), oxidation state of sulfur is -2. e) Sulfuric Acid: \(\mathrm{H_2SO_4}\), oxidation state of sulfur is +6. f) Sulfur Dioxide: \(\mathrm{SO_2}\), oxidation state of sulfur is +4. g) Mercury Telluride: \(\mathrm{HgTe}\), oxidation state of tellurium is -2.

Step by step solution

01

Write the chemical formula

The Group 6A element in sulfur tetrachloride is sulfur (S). It's combined with four chlorine (Cl) atoms. Thus, the chemical formula is \(S\mathrm{Cl_4}\).
02

Determine the oxidation state of sulfur

In compounds, the oxidation state of chlorine is generally -1. Since there are four chlorine atoms, the total charge from chlorine is -4. For the compound to be neutral, sulfur must have an oxidation state of +4. Therefore, the oxidation state of sulfur is +4. #b) Selenium Trioxide#
03

Write the chemical formula

The Group 6A element in selenium trioxide is selenium (Se). It's combined with three oxygen (O) atoms. Thus, the chemical formula is \(\mathrm{SeO_3}\).
04

Determine the oxidation state of selenium

In compounds, the oxidation state of oxygen is generally -2. Since there are three oxygen atoms, the total charge from oxygen is -6. For the compound to be neutral, selenium must have an oxidation state of +6. Therefore, the oxidation state of selenium is +6. #c) Sodium Thiosulfate#
05

Write the chemical formula

Sodium thiosulfate is a compound consisting of two sodium (Na) ions, one sulfur (S) atom, and three oxygen (O) atoms, with the Group 6A element being sulfur (S). Thus, the chemical formula is \(\mathrm{Na_2S_2O_3}\).
06

Determine the oxidation state of sulfur

Sodium has an oxidation state of +1 and each of the three oxygen atoms has an oxidation state of -2. That gives a total charge of +2 for sodium and -6 for the oxygen atoms. To balance the oxygen charges, the two sulfur atoms must have a total oxidation state of +4. This gives an average oxidation state of +2 for each sulfur atom in sodium thiosulfate. #d) Hydrogen Sulfide#
07

Write the chemical formula

Hydrogen sulfide consists of a sulfur (S) atom and two hydrogen (H) atoms. Thus, the chemical formula is \(\mathrm{H_2S}\).
08

Determine the oxidation state of sulfur

Hydrogen has an oxidation state of +1. Since there are two hydrogen atoms, the total charge from hydrogen is +2. For the compound to be neutral, sulfur must have an oxidation state of -2. Therefore, the oxidation state of sulfur is -2. #e) Sulfuric Acid#
09

Write the chemical formula

Sulfuric acid consists of a sulfur (S) atom, four oxygen (O) atoms, and two hydrogen (H) atoms. Thus, the chemical formula is \(\mathrm{H_2SO_4}\).
10

Determine the oxidation state of sulfur

Hydrogen has an oxidation state of +1, and oxygen has an oxidation state of -2. Since there are two hydrogen atoms and four oxygen atoms, the total charge from hydrogen is +2 and the total charge from oxygen is -8. For the compound to be neutral, sulfur must have an oxidation state of +6. Therefore, the oxidation state of sulfur is +6. #(f) Sulfur Dioxide#
11

Write the chemical formula

Sulfur dioxide consists of a sulfur (S) atom and two oxygen (O) atoms. Thus, the chemical formula is \(\mathrm{SO_2}\).
12

Determine the oxidation state of sulfur

Oxygen has an oxidation state of -2. Since there are two oxygen atoms, the total charge from oxygen is -4. For the compound to be neutral, sulfur must have an oxidation state of +4. Therefore, the oxidation state of sulfur is +4. #g) Mercury Telluride#
13

Write the chemical formula

Mercury telluride consists of mercury (Hg) and tellurium (Te), with tellurium being the Group 6A element. Thus, the chemical formula is \(\mathrm{HgTe}\).
14

Determine the oxidation state of tellurium

Mercury has an oxidation state of +2. For the compound to be neutral, tellurium must have an oxidation state of -2. Therefore, the oxidation state of tellurium is -2.

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Most popular questions from this chapter

An aqueous solution of \(\mathrm{SO}_{2}\) reduces (a) aqueous \(\mathrm{KMnO}_{4}\) to \(\mathrm{MnSO}_{4}(a q),(\mathbf{b})\) acidic aqueous \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) to aqueous \(\mathrm{Cr}^{3+}\) (\mathbf{c} ) \text { aqueous } \mathrm { Hg } _ { 2 } ( \mathrm { NO } _ { 3 } ) _ { 2 } \text { to mercury metal. Write balanced } equations for these reactions.

(a) How many grams of \(\mathrm{H}_{2}\) can be stored in 100.0 \(\mathrm{kg}\) of the alloy FeTi if the hydride FeTiH_ is formed? (b) What volume does this quantity of \(\mathrm{H}_{2}\) occupy at STP? (c) If this quantity of hydrogen was combusted in air to produce liquid water, how much energy could be produced?

Write a balanced equation for each of the following reactions: (a) preparation of white phosphorus from calcium phosphate, (b) hydrolysis of PBry, (c) reduction of PBr_ to \(P_{4}\) in the gas phase, using \(\mathrm{H}_{2}\) .

Write the chemical formula for each of the following compounds, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) chlorate ion, (b) hydroiodic acid, (c) iodine trichloride, (d) sodium hypochlorite, (e) perchloric acid, (f) xenon tetrafluoride.

Complete and balance the following equations:$$\begin{array}{l}{\text { (a) } \mathrm{Mg}_{3} \mathrm{N}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { (b) } \mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow} \\ {\text { (c) } \mathrm{MnO}_{2}(s)+\mathrm{C}(s) \stackrel{\Delta}{\longrightarrow}}\end{array}$$ $$\begin{array}{l}{\text { (d) } \operatorname{AlP}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { (e) } \mathrm{Na}_{2} \mathrm{S}(s)+\mathrm{HCl}(a q) \longrightarrow}\end{array}$$
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