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Chapter 4: Problem 49

Determine the oxidation number for the indicated element in each of the following substances: (a) \(\mathrm{S}\) in \(\mathrm{SO}_{2},\) (b) \(\mathrm{C}\) in \(\mathrm{COCl}_{2}\), (c) \(\mathrm{Mn}\) in \(\mathrm{KMnO}_{4}\) (d) \(\mathrm{Br}\) in \(\mathrm{HBrO}\) (e) As in As \(_{4}\), (f) \(\mathrm{O}\) in \(\mathrm{K}_{2} \mathrm{O}_{2}\)

Short Answer

Expert verified
(a) The oxidation number of $\mathrm{S}$ in $\mathrm{SO}_{2}$ is +4. (b) The oxidation number of $\mathrm{C}$ in $\mathrm{COCl}_{2}$ is +4. (c) The oxidation number of $\mathrm{Mn}$ in $\mathrm{KMnO}_{4}$ is +7. (d) The oxidation number of $\mathrm{Br}$ in $\mathrm{HBrO}$ is +1. (e) The oxidation number of As in As$_{4}$ is 0. (f) The oxidation number of $\mathrm{O}$ in $\mathrm{K}_{2} \mathrm{O}_{2}$ is -1.

Step by step solution

01

(a) Determine the oxidation number of S in SO2

To find the oxidation number of S in SO2, we need to consider the oxidation numbers of the other elements in the compound. Oxygen generally has an oxidation number of -2. Thus, in SO2, there are two oxygen atoms, each with an oxidation number of -2, contributing a total of -4. Therefore, in SO2, the oxidation number of S must be +4 to balance out the contribution from the oxygen atoms.
02

(b) Determine the oxidation number of C in COCl2

For COCl2, let's first focus on the Cl atoms. Chlorine generally has an oxidation number of -1. Since there are two Cl atoms, they have a combined oxidation number of -2. Oxygen has an oxidation number of -2 as well. So, to balance the oxidation numbers, the C atom must have an oxidation number of +4.
03

(c) Determine the oxidation number of Mn in KMnO4

In KMnO4, we can see that K is a Group 1 metal, which generally has an oxidation number of +1. Oxygen is -2, and there are four oxygen atoms, with a total oxidation number of -8. To achieve an overall charge of zero, Mn must have an oxidation number of +7.
04

(d) Determine the oxidation number of Br in HBrO

In HBrO, we already know that the oxidation number of H is +1 and the oxidation number of O is -2. To balance the oxidation state and achieve overall charge of zero, the oxidation number of Br in HBrO must be +1.
05

(e) Determine the oxidation number of As in As4

In a pure elemental form, such as As in As4, the oxidation number is always zero. Hence, the oxidation number of As in As4 is 0.
06

(f) Determine the oxidation number of O in K2O2

In K2O2, there are two K atoms, each with an oxidation number of +1, contributing a total oxidation number of +2. Peroxide, O2^2-, generally has an oxidation number of -1 for each oxygen atom, making the total for two O atoms -2. As a result, the oxidation number of O in K2O2 is -1.

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