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Chapter 4: Problem 48

Determine the oxidation number of sulfur in each of the following substances: (a) barium sulfate, \(\mathrm{BaSO}_{4},\) (b) sulfurous acid, $\mathrm{H}_{2} \mathrm{SO}_{3},(\mathbf{c})\( strontium sulfide, \)\mathrm{Sr} S,(\mathbf{d})$ hydrogen sulfide, \(\mathrm{H}_{2} \mathrm{~S}\). (e) Locate sulfur in the periodic table in Exercise 4.47 what region is it in? (f) Which region(s) of the periodic table contains elements that can adopt both positive and negative oxidation numbers?

Short Answer

Expert verified
The oxidation number of sulfur (S) in given compounds is: (a) In barium sulfate (BaSO4), the oxidation number of S is \(+6\). (b) In sulfurous acid (H2SO3), the oxidation number of S is \(+4\). (c) In strontium sulfide (SrS), the oxidation number of S is \(-2\). (d) In hydrogen sulfide (H2S), the oxidation number of S is \(-2\). Sulfur is located in the p-block and the nonmetals' group in the periodic table (period 3 and group 16). Elements with both positive and negative oxidation numbers are mainly found in the p-block, which includes nonmetals, metalloids, and post-transition metals.

Step by step solution

01

Recall oxidation number rules

In order to determine the oxidation numbers of sulfur in the given compounds, it is important to remember the following rules: 1. The oxidation number of an element in its elemental form is 0. 3. The oxidation number of an alkali metal (Group 1) is +1, and for an alkaline earth metal (Group 2), it is +2. 2. The oxidation number of hydrogen is usually +1 in its compounds, except in metal hydrides where it is -1. 4. The oxidation number of oxygen is usually -2, except in peroxides, where it is -1 or in the presence of fluorine.
02

Determine the oxidation number of sulfur in barium sulfate (BaSO4)

In BaSO4, Ba is an alkaline earth metal (Group 2), so its oxidation number is +2. Oxygen has an oxidation number of -2. Since the compound is neutral, the oxidation number of sulfur can be calculated using the equation: +2 (Ba) + x (S) + 4(-2) (O) = 0 Solve for x: 2 + x - 8 = 0 x = +6 Therefore, the oxidation number of sulfur in BaSO4 is \(+6\).
03

Determine the oxidation number of sulfur in sulfurous acid (H2SO3)

In H2SO3, hydrogen has an oxidation number of +1, and there are two hydrogen atoms in the compound. Oxygen has an oxidation number of -2. Using the equation: 2(+1) (H) + x (S) + 3(-2) (O) = 0 Solve for x: 2 + x - 6 = 0 x = +4 Therefore, the oxidation number of sulfur in H2SO3 is \(+4\).
04

Determine the oxidation number of sulfur in strontium sulfide (SrS)

In SrS, Sr is an alkaline earth metal with an oxidation number of +2. The compound is neutral, so we can use the equation: +2 (Sr) + x (S) = 0 Solve for x: 2 + x = 0 x = -2 Therefore, the oxidation number of sulfur in SrS is \(-2\).
05

Determine the oxidation number of sulfur in hydrogen sulfide (H2S)

In H2S, hydrogen has an oxidation number of +1, and there are two hydrogen atoms in the compound. The equation for the oxidation number of sulfur is: 2(+1) (H) + x (S) = 0 Solve for x: 2 + x = 0 x = -2 Therefore, the oxidation number of sulfur in H2S is \(-2\).
06

Locate sulfur in the periodic table and identify its region

Sulfur is in period 3 and group 16 (also known as Group VIA) of the periodic table. It belongs to the p-block and the nonmetals' group.
07

Discuss which regions of the periodic table have elements with both positive and negative oxidation numbers

The elements that have both positive and negative oxidation numbers can be found mainly in the p-block of the periodic table. This group includes nonmetals, metalloids, and post-transition metals.

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Most popular questions from this chapter

A \(0.5895-\mathrm{g}\) sample of impure magnesium hydroxide is dissolved in \(100.0 \mathrm{~mL}\) of \(0.2050 \mathrm{MHCl}\) solution. The excess acid then needs \(19.85 \mathrm{~mL}\) of \(0.1020 \mathrm{M} \mathrm{NaOH}\) for neutralization. Calculate the percentage by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the HCl solution.

Which element is oxidized, and which is reduced in the following reactions? (a) $\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$ (b) $3 \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{Al}(s) \longrightarrow$ $$ 3 \mathrm{Fe}(s)+2 \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q) $$ (c) $\mathrm{Cl}_{2}(a q)+2 \mathrm{NaI}(a q) \longrightarrow \mathrm{I}_{2}(a q)+2 \mathrm{NaCl}(a q)$ (d) $\mathrm{PbS}(s)+4 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)+4 \mathrm{H}_{2} \mathrm{O}(I)$

Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) \(\mathrm{Hg}_{2} \mathrm{SO}_{4}\) (b) \(\mathrm{NH}_{4} \mathrm{OH}\), (c) \(\mathrm{Ni}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\) (d) \(\mathrm{AgNO}_{3}\), (e) FeCO \(_{3}\)

Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid, (b) chromium with hydrobromic acid, (c) tin with hydrochloric acid, (d) aluminum with formic acid, \(\mathrm{HCOOH}\).

Consider the following reagents: zinc, copper, mercury (density $13.6 \mathrm{~g} / \mathrm{mL}$ ), silver nitrate solution, nitric acid solution. (a) Given a \(500-\mathrm{mL}\). Erlenmeyer flask and a balloon, can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a balanced chemical equation to represent this process. What is the identity of the substance that inflates the balloon? (b) What is the theoretical yield of the substance that fills the balloon? (c) Can you combine two or more of the foregoing reagents to initiate a chemical reaction that will produce metallic silver? Write a balanced chemical equation to represent this process. What ions are left behind in solution? (d) What is the theoretical yield of silver?
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