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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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Most popular questions from this chapter

Using the standard reduction potentials listed in Appendix E, calculate the equilibrium constant for each of the following reactions at \(298 \mathrm{~K}\) : (a) $\mathrm{Cu}(s)+2 \mathrm{Ag}^{+}(a q) \longrightarrow \mathrm{Cu}^{2+}(a q)+2 \mathrm{Ag}(s)$ (b) $3 \mathrm{Ce}^{4+}(a q)+\mathrm{Bi}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 3 \mathrm{Ce}^{3+}(a q)+ \mathrm{BiO}^{+}(a q)+2 \mathrm{H}^{+}(a q)$ (c) $\mathrm{N}_{2} \mathrm{H}_{5}^{+}(a q)+4 \mathrm{Fe}(\mathrm{CN})_{6}^{3-}(a q) \longrightarrow \mathrm{N}_{2}(g)+ 5 \mathrm{H}^{+}(a q)+4 \mathrm{Fe}(\mathrm{CN})_{6}^{4-}(a q)$

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