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Chapter 17: Problem 14

Assign oxidation numbers to the atoms in the ionic compound \(\mathrm{NH}_{4} \mathrm{NO}_{3}(s) .\)

Short Answer

Expert verified
The oxidation numbers of the atoms in \(NH_4NO_3(s)\) are: Nitrogen -3 and +5, Hydrogen +1, and Oxygen -2.

Step by step solution

01

Identify Oxidation Number Rules

The rules for assigning oxidation numbers to atoms are as follows: 1) The oxidation number of an atom in its elemental state is zero. 2) The oxidation number of a monatomic ion equals the charge of the ion. 3) The oxidation number of hydrogen in a compound is usually +1. 4) Oxygen in a compound has the oxidation number of -2.
02

Assign Oxidation Numbers for the Ammonium Ion

Starting with the ammonium ion, \(NH_4^+\), each hydrogen atom has an oxidation number of +1 because it is in a compound. This means the nitrogen in this ion has to have an oxidation number of -3 because the sum of the oxidation numbers in a neutral compound must be zero and in an ion, they must equal the charge of the ion. Here, +1*4 from hydrogen and -3 from nitrogen equals +1, the charge of the ion.
03

Assign Oxidation Numbers for the Nitrate Ion

Next is the nitrate ion, \(NO_3^-\). Each oxygen atom has an oxidation number of -2 because it is in a compound, so collectively, they contribute -6. This means the nitrogen in this ion has to have an oxidation number of +5 because the sum of the oxidation numbers in an ion must equal the charge of the ion. Here, -2*3 from the oxygen and +5 from nitrogen equals -1, the charge of the ion.

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Most popular questions from this chapter

Explain how oxidation numbers are used to identify redox reactions?

How does the oxidation number of an atom of Mn change in the reaction below? $$\begin{array}{r}{4 \mathrm{Mn}^{2+}(a q)+\mathrm{MnO}_{4}^{-}(a q)+8 \mathrm{H}_{3} \mathrm{O}^{+}(a q)+} \\ {15 \mathrm{H}_{2} \mathrm{P}_{4} \mathrm{O}_{7}^{2-}(a q) \rightarrow 12 \mathrm{H}_{2} \mathrm{O}(l)+} \\\ {\quad 5 \mathrm{Mn}\left(\mathrm{H}_{2} \mathrm{P}_{4} \mathrm{O}_{7}\right)_{3}^{3-}(a q)}\end{array}$$

Carpentry nails are steel, but some are plated with a second metal. Obtain a variety of nails and evaluate their tendency to rust by laying them on a piece of cloth moistened by water containing salt and vinegar, so they are exposed both to the liquid and to air. After two weeks, report your findings.

In an electrochemical cell, what role does the porous barrier play? What would happen without it?

Calculate the Equilibrium Constant, using the Standard Cell Voltage The graphing calculator can run a program that calculates the equilibrium constant for an electrochemical cell using an equation called the Nernst equation, given the standard potential and the number of electrons transferred. Given that the standard potential is 2.041 V and that two electrons are transferred, you will calculate the equilibrium constant. The program will be used to make the calculations. Go to Appendix c. If you are using a TI-83 Plus, you can download the program NERNST and data and run the application as directed. If you are using another calculator, your teacher will provide you with key- strokes and data sets to use. After you have run the program, answer the following questions. \begin{equation} \begin{array}{l}{\text { a. What is the equilibrium constant when }} \\\ {\text { the standard potential is } 0.099 ?} \\ {\text { b. What is the equilibrium constant when }} \\ {\text { the standard potential is } 1.125 ?} \\\ {\text { c. What is the equilibrium constant when }} \\ {\text { the standard potential is } 2.500 ?}\end{array} \end{equation}
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