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Chapter 22: Problem 52

Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) nitric oxide, (b) hydrazine, (c) potassium cyanide, (d) sodium nitrite, (e) ammonium chloride, (f) lithium nitride.

Short Answer

Expert verified
(a) Nitric oxide: NO, oxidation state of N: +2 (b) Hydrazine: N2H4, oxidation state of N: -2 (c) Potassium cyanide: KCN, oxidation state of N: -3 (d) Sodium nitrite: NaNO2, oxidation state of N: +3 (e) Ammonium chloride: NH4Cl, oxidation state of N: -3 (f) Lithium nitride: Li3N, oxidation state of N: -3

Step by step solution

01

(a) Nitric Oxide

Nitric oxide contains nitrogen (N) and oxygen (O). The chemical symbol for nitrogen is N, and the chemical symbol for oxygen is O. In nitric oxide, nitrogen has an oxidation state of +2, and the oxygen has an oxidation state of -2. The chemical formula for nitric oxide is NO.
02

(b) Hydrazine

Hydrazine is composed of nitrogen (N) and hydrogen (H). The chemical symbol for nitrogen is N, while the chemical symbol for hydrogen is H. In hydrazine, nitrogen has an oxidation state of -2 and hydrogen has an oxidation state of +1. The chemical formula for hydrazine is N2H4.
03

(c) Potassium Cyanide

Potassium cyanide consists of potassium (K) and a cyanide ion (CN). The chemical symbol for potassium is K, and the chemical symbol for the cyanide ion is CN. In potassium cyanide, the potassium ion has a charge of +1, while the cyanide ion has a charge of -1. The nitrogen in the cyanide ion has an oxidation state of -3. The chemical formula for potassium cyanide is KCN.
04

(d) Sodium Nitrite

Sodium nitrite is composed of sodium (Na) and a nitrite ion (NO2). The chemical symbol for sodium is Na, while the chemical symbol for the nitrite ion is NO2. In sodium nitrite, the sodium ion has a charge of +1, and the nitrite ion has a charge of -1. The nitrogen in the nitrite ion has an oxidation state of +3. The chemical formula for sodium nitrite is NaNO2.
05

(e) Ammonium Chloride

Ammonium chloride consists of an ammonium ion (NH4) and a chloride ion (Cl). The chemical symbol for the ammonium ion is NH4, and the chemical symbol for the chloride ion is Cl. In ammonium chloride, the ammonium ion has a charge of +1, and the chloride ion has a charge of -1. The nitrogen in the ammonium ion has an oxidation state of -3. The chemical formula for ammonium chloride is NH4Cl.
06

(f) Lithium Nitride

Lithium nitride is composed of lithium (Li) and nitrogen (N). The chemical symbol for lithium is Li, and the chemical symbol for nitrogen is N. In lithium nitride, lithium has an oxidation state of +1, while nitrogen has an oxidation state of -3. The chemical formula for lithium nitride is Li3N.

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Most popular questions from this chapter

Are the physical properties of \(\mathrm{H}_{2} \mathrm{O}\) different from \(\mathrm{D}_{2} \mathrm{O}\) ? Explain.

The standard heats of formation of \(\mathrm{H}_{2} \mathrm{O}(g), \mathrm{H}_{2} \mathrm{~S}(g), \mathrm{H}_{2} \mathrm{Se}(g)\), and \(\mathrm{H}_{2} \mathrm{Te}(g)\) are \(-241.8,-20.17,+29.7\), and \(+99.6 \mathrm{~kJ} /\) mol, respectively. The enthalpies necessary to convert the elements in their standard states to one mole of gaseous atoms are \(248,277,227\), and \(197 \mathrm{~kJ} / \mathrm{mol}\) of atoms for \(\mathrm{O}, \mathrm{S}, \mathrm{Se}\), and Te, respectively. The enthalpy for dissociation of \(\mathrm{H}_{2}\) is \(436 \mathrm{~kJ} / \mathrm{mol}\). Calculate the average \(\mathrm{H}-\mathrm{O}, \mathrm{H}-\mathrm{S}, \mathrm{H}-\mathrm{Se}\), and \(\mathrm{H}\) - Te bond enthalpies, and comment on their trend.

SOLUTION Analyze We must write balanced nuclear equations in which the masses and charges of reactants and products are equal. Plan We can begin by writing the complete chemical symbols for the nuclei and decay particles that are given in the problem. Solve (a) The information given in the question can be summarized as $$ { }_{80}^{201} \mathrm{Hg}+{ }_{-1}^{0} \mathrm{e} \longrightarrow{ }_{Z}^{A} \mathrm{X} $$ The mass numbers must have the same sum on both sides of the equation: $$ 201+0=A $$ Thus, the product nucleus must have a mass number of 201. Similarly, balancing the atomic numbers gives $$ 80-1=Z $$ Thus, the atomic number of the product nucleus must be 79 , which identifies it as gold (Au): $$ { }_{80}^{201} \mathrm{Hg}+{ }_{-1}^{0} \mathrm{e} \longrightarrow{ }_{79}^{201} \mathrm{Au} $$ (b) In this case we must determine what type of particle is emitted in the course of the radioactive decay: $$ { }_{90}^{231} \mathrm{Th} \longrightarrow{ }_{91}^{231} \mathrm{~Pa}+{ }_{\mathrm{Z}}^{\mathrm{X}} \mathrm{X} $$ From \(231=231+A\) and \(90=91+Z\), we deduce \(A=0\) and \(Z=-1\). According to Table \(21.2\), the particle with these characteristics is the beta particle (electron). We therefore write $$ { }_{90}^{231} \mathrm{Th} \longrightarrow{ }_{91}^{231} \mathrm{~Pa}+{ }_{-1}^{0} \mathrm{e} \text { or } \quad{ }_{90}^{231} \mathrm{Th} \longrightarrow{ }_{91}^{231} \mathrm{~Pa}+\beta^{-} $$

Write balanced equations for each of the following reactions (some of these are analogous to reactions shown in the chapter). (a) Aluminum metal rcacts with acids to form hydrogen gas. (b) Steam reacts with magnesium metal to give magnesium oxide and hydrogen. (c) Manganese(IV) oxide is reduced to manganesc(II) oxide by hydrogen gas. (d) Calcium hydride reacts with water to generate hydrogen gas.

Write balanced equations for each of the following reactions. (a) When mercury(II) oxide is heated, it decomposes to form \(\mathrm{O}_{2}\) and mercury metal. (b) When copper(II) nitrate is heated strongly, it decomposes to form copper(II) oxide, nitrogen dioxide, and oxygen. (c) Lead(II) sulfide, \(\mathrm{PbS}(s)\), reacts with ozone to form \(\mathrm{PbSO}_{4}(s)\) and \(\mathrm{O}_{2}(g)\). (d) When heated in air, \(\mathrm{ZnS}(s)\) is converted to \(\mathrm{ZnO}\). (e) Potassium peroxide reacts with \(\mathrm{CO}_{2}(g)\) to give potassium carbonate and \(\mathrm{O}_{2}\) (f) Oxygen is converted to ozone in the upper atmosphere.
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