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Chapter 20: Problem 113

Aqueous solutions of ammonia \(\left(\mathrm{NH}_{3}\right)\) and bleach (active ingredient \(\mathrm{NaOCl}\) ) are sold as cleaning fluids, but bottles of both of them warn: "Never mix ammonia and bleach, as toxic gases may be produced." One of the toxic gases that can be produced is chloroamine, \(\mathrm{NH}_{2} \mathrm{Cl}\). (a) What is the oxidation number of chlorine in bleach? (b) What is the oxidation number of chlorine in chloramine? (c) Is Cl oxidized, reduced, or neither, upon the conversion of bleach to chloramine? (d) Another toxic gas that can be produced is nitrogen trichloride, \(\mathrm{NCl}_{3}\). What is the oxidation number of \(\mathrm{N}\) in nitrogen trichloride? \((\mathbf{e})\) Is \(\mathrm{N}\) oxidized, reduced, or neither, upon the conversion of ammonia to nitrogen trichloride?

Short Answer

Expert verified
(a) The oxidation number of Cl in bleach (NaOCl) is +1. (b) The oxidation number of Cl in chloroamine (NH2Cl) is +1. (c) Cl is neither oxidized nor reduced upon the conversion of bleach to chloroamine. (d) The oxidation number of N in nitrogen trichloride (NCl3) is +3. (e) N is oxidized upon the conversion of ammonia to nitrogen trichloride.

Step by step solution

01

(a) Oxidation number of Cl in NaOCl (bleach)

To find the oxidation number of Cl in NaOCl (bleach), we will first look at the oxidation numbers of the other elements in the compound. Na is an alkali metal and has an oxidation number of +1, while O generally has an oxidation number of -2. Now we can create an equation to represent the total oxidation numbers of the compound: \[+1 + (-2) + x = 0\] \[x = +1\] Therefore, the oxidation number of Cl in bleach (NaOCl) is +1.
02

(b) Oxidation number of Cl in NH2Cl (chloroamine)

To find the oxidation number of Cl in NH2Cl (chloroamine), we first look at the oxidation numbers of the other elements in the compound. N usually has an oxidation number of -3, while H has an oxidation number of +1. Since there are two H atoms in the compound, we can create an equation to represent the total oxidation numbers of the compound: \[(-3) + 2(+1) + x = 0\] \[-3 + 2 + x = 0\] \[x = +1\] Therefore, the oxidation number of Cl in chloroamine (NH2Cl) is +1.
03

(c) Cl's oxidation state during conversion from NaOCl to NH2Cl

Comparing the oxidation numbers of Cl in NaOCl (bleach) and NH2Cl (chloroamine), which are both +1, we can determine that during the conversion of bleach to chloroamine, the oxidation number of Cl remains the same. Thus, Cl is neither oxidized nor reduced in this process.
04

(d) Oxidation number of N in NCl3 (nitrogen trichloride)

To find the oxidation number of N in NCl3 (nitrogen trichloride), we first look at the oxidation number of Cl, which is typically -1. Since there are three Cl atoms in the compound, we can create an equation to represent the total oxidation numbers of the compound: \[x + 3(-1) = 0\] \[x - 3 = 0\] \[x = +3\] Therefore, the oxidation number of N in nitrogen trichloride (NCl3) is +3.
05

(e) N's oxidation state during conversion from NH3 to NCl3

Comparing the oxidation numbers of N in NH3 (ammonia) and NCl3 (nitrogen trichloride), which are -3 and +3 respectively, we can determine that during the conversion of ammonia to nitrogen trichloride, the oxidation number of N increases from -3 to +3. Thus, N is oxidized in this process.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Oxidation State
Oxidation state, or oxidation number, is a concept used to keep track of electrons in molecules and ions, especially during chemical reactions. It indicates the hypothetical charge of an atom if all bonds to atoms of different elements were 100% ionic. Understanding oxidation states is crucial because they help us identify changes in electron distribution during chemical reactions.

For instance, in the compound NaOCl (bleach), the oxidation state of chlorine (Cl) is +1. This is calculated by knowing that sodium (Na) typically has an oxidation state of +1 and oxygen (O) is -2. The sum of these oxidation states must equal zero in a neutral compound. We set up the equation: \[+1 + (-2) + x = 0\] This simplifies to \(x = +1\), making chlorine's oxidation state in NaOCl +1.
Reduction and Oxidation Reactions
Reduction and oxidation reactions, often abbreviated as redox reactions, represent a type of chemical reaction where the oxidation numbers of atoms are altered. In these reactions, the substance that gains electrons is said to be reduced, whereas the one losing electrons is oxidized.

With the conversion of bleach (NaOCl) to chloroamine (NH2Cl), the oxidation state of chlorine remains unchanged at +1, indicating that chlorine is neither oxidized nor reduced in this process. However, in another reaction involving ammonia converting to nitrogen trichloride \( (NCl_3) \), nitrogen experiences a change in oxidation state from -3 to +3, signifying that nitrogen is oxidized.

Redox reactions are fundamental to many biological processes and chemical industry applications. They are crucial for energy production, whether in photosynthesis or cellular respiration.
Chemical Reactions Safety
Chemical reactions can sometimes result in hazardous conditions if not performed safely. Understanding the components and products involved in chemical reactions can prevent dangerous situations.

A classic example of a chemical safety warning is the mixture of ammonia \((NH_3)\) and bleach \((NaOCl)\). These two common household cleaners, when mixed, can produce toxic gases, including chloramine \((NH_2Cl)\) and nitrogen trichloride \((NCl_3)\).
  • The primary recommendation for safe chemical handling is to always read and follow label warnings and instructions on all products.
  • Ensure proper ventilation, use protective gear such as gloves and goggles, and avoid mixing unknown chemicals.
These precautions can minimize risks and protect against exposure to toxic materials.
Toxic Gas Production
When ammonia and bleach are mixed, one of the dangerous outcomes is toxic gas production. These gases can pose serious health dangers if inhaled or contacted.

Chloramine \((NH_2Cl)\) is one such toxic gas that is produced when the two chemicals interact. It can cause respiratory issues and irritation to the eyes and skin. Another dangerous compound that might form is nitrogen trichloride \( (NCl_3) \). Nitrogen trichloride is even more hazardous, with potential to cause severe health problems on exposure.
  • The best prevention is to avoid mixing cleaning agents unless sure of the absence of harmful reactions.
  • If exposure occurs, it's crucial to move to fresh air immediately and seek medical attention if symptoms persist.
Understanding how these gases are produced can help prevent accidental exposure and safeguard health.

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Most popular questions from this chapter

(a) Suppose that an alkaline battery was manufactured using cadmium metal rather than zinc. What effect would this have on the cell emf? (b) What environmental advantage is provided by the use of nickel-metal hydride batteries over nickel-cadmium batteries?

(a) Aluminum metal is used as a sacrificial anode to protect offshore pipelines in salt water from corrosion. Why is the aluminum referred to as a "sacrificial anode"? (b) Looking in Appendix E, suggest what metal the pipelines could be made from in order for aluminum to be successful as a sacrificial anode.

The standard reduction potentials of the following half-reactions are given in Appendix E: $$ \begin{array}{l} \mathrm{Fe}^{2+}(a q)+2 \mathrm{e}^{-} \longrightarrow \mathrm{Fe}(s) \\ \mathrm{Cd}^{2+}(a q)+2 \mathrm{e}^{-} \longrightarrow \operatorname{Cd}(s) \\\ \mathrm{Sn}^{2+}(a q)+2 \mathrm{e}^{-} \longrightarrow \operatorname{Sn}(s) \\\ \mathrm{Ag}^{+}(a q)+\mathrm{e}^{-} \longrightarrow \operatorname{Ag}(s) \end{array} $$ (a) Determine which combination of these half-cell reactions leads to the cell reaction with the largest positive cell potential and calculate the value. (b) Determine which combination of these half-cell reactions leads to the cell reaction with the smallest positive cell potential and calculate the value.

Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (a) \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q) \longrightarrow \mathrm{Cr}^{3+}(a q)\) (acidic solution) (b) \(\mathrm{Mn}^{2+}(a q) \longrightarrow \mathrm{MnO}_{4}^{-}(a q)\) (acidic solution) (c) \(\mathrm{I}_{2}(s) \longrightarrow \mathrm{IO}_{3}^{-}(a q)\) (acidic solution) (d) \(\mathrm{S}(s)(a q) \longrightarrow \mathrm{H}_{2} \mathrm{~S}(g)\) (acidic solution) (e) \(\mathrm{NO}_{3}^{-}(a q) \longrightarrow \mathrm{NO}_{2}^{-}(a q)\) (basic solution) (f) \(\mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{OH}^{-}(a q)\) (basic solution)

A voltaic cell similar to that shown in Figure 20.5 is constructed. One electrode half-cell consists of a magnesium strip placed in a solution of \(\mathrm{MgCl}_{2}\), and the other has a nickel strip placed in a solution of \(\mathrm{NiCl}_{2}\). The overall cell reaction is $$ \mathrm{Mg}(s)+\mathrm{Ni}^{2+}(a q) \longrightarrow \mathrm{Ni}(s)+\mathrm{Mg}^{2+}(a q) $$ (a) What is being oxidized, and what is being reduced? (b) Write the half- reactions that occur in the two half-cells. (c) Which electrode is the anode, and which is the cathode?(d) Indicate the signs of the electrodes. (e) Do electrons flow from the magnesium electrode to the nickel electrode or from the nickel to the magnesium? (f) In which directions do the cations and anions migrate through the solution?
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