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Chapter 4: Problem 41

Arrange the following species in order of increasing oxidation number of the sulfur atom: (a) \(\mathrm{H}_{2} \mathrm{~S}\) (b) \(\mathrm{S}_{8}\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (d) \(\mathrm{S}^{2-},(\mathrm{e}) \mathrm{HS}^{-},(\mathrm{f}) \mathrm{SO}_{2},(\mathrm{~g}) \mathrm{SO}_{3}\)

Short Answer

Expert verified
So, the species in increasing order of oxidation number of sulfur are: \(S_{8}\) (-2), \(H_{2}S\) (-1), \(HS^{-}\) (+4), \(SO_{2}\) (+6), \(H_{2}SO_{4}\), \(SO_{3}\)

Step by step solution

01

Oxidation Number for H2S

In H2S, Hydrogen has an oxidation number of +1. Since there are two, the total is +2. In order to balance this, Sulphur's oxidation number must be -2.
02

Oxidation Number for S8

In S8, Sulfur is in its elemental form, so its oxidation number is zero.
03

Oxidation Number for H2SO4

In H2SO4, Hydrogen's oxidation number is +1 and Oxygen's is -2. Since there are two hydrogen atoms and four oxygen atoms, the total is +2 -8 = -6. To balance this, Sulfur's oxidation number must be +6.
04

Oxidation Number for S^2-

In S^2-, Sulfur is in the form of an ion. So, its oxidation number is -2, which is equal to its charge.
05

Oxidation Number for HS^-

In HS^-, Hydrogen's oxidation number is +1. Since the compound is negative, to balance the charge, Sulphur's oxidation number must be -1.
06

Oxidation Number for SO2

In SO2, Oxygen's oxidation number is -2. Since there are two oxygen atoms, the total is -4. To balance this, Sulphur's oxidation number must be +4.
07

Oxidation Number for SO3

In SO3, Oxygen's oxidation number is -2. Since there are three oxygen atoms, the total is -6. To balance this, Sulphur's oxidation number must be +6.

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Most popular questions from this chapter

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