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Chapter 22: Problem 49

Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: (a) sodium azide, (b) ammonium ion, (c) nitrous acid, \((\mathbf{d})\) magnesium nitride, \((\mathbf{e})\) diazene, \((\mathbf{f})\) sodium nitrate, (g) nitrogen trifluoride, (h) nitric acid.

Short Answer

Expert verified
\( (a) \: NaN_3 \: (N: -\frac{1}{3}) \newline (b) \: NH_4^+ \: (N: -3) \newline (c) \: HNO_2 \: (N: +3) \newline (d) \: Mg_3N_2 \: (N: -3) \newline (e) \: N_2H_2 \: (N: -1) \newline (f) \: NaNO_3 \: (N: +5) \newline (g) \: NF_3 \: (N: +3) \newline (h) \: HNO_3 \: (N: +5) \)

Step by step solution

01

(a) Sodium Azide

Sodium azide has the chemical formula NaN₃. The azide ion (N₃⁻) has an overall charge of -1, and the sodium ion (Na⁺) has a charge of +1. Therefore, the oxidation state of nitrogen in sodium azide is -1/3 since there are three nitrogen atoms, and the overall charge of the azide ion is -1.
02

(b) Ammonium Ion

The ammonium ion has the chemical formula NH₄⁺. In this ion, nitrogen is bonded to four hydrogen atoms, each having an oxidation state of +1. The nitrogen atom has an oxidation state of -3 because the total charge of the ammonium ion is +1, and there are four hydrogen atoms with a combined oxidation state of +4.
03

(c) Nitrous Acid

Nitrous acid has the chemical formula HNO₂. In this molecule, the nitrogen atom is bonded to one hydrogen atom (oxidation state +1) and two oxygen atoms (oxidation state -2 each). The oxidation state of nitrogen in nitrous acid is +3 because the total charge of the molecule is 0, and the nitrogen atom balances the charges of the surrounding atoms.
04

(d) Magnesium Nitride

Magnesium nitride has the chemical formula Mg₃N₂. In this compound, three magnesium atoms (oxidation state +2 each) are bonded to two nitrogen atoms (oxidation state -3 each). Since there are two nitrogen atoms and the overall charge of the molecule is 0, the oxidation state of each nitrogen atom in magnesium nitride is -3.
05

(e) Diazene

Diazene has the chemical formula N₂H₂. In diazene, two nitrogen atoms (each sharing a double bond with each other) are bonded to one hydrogen atom each. The oxidation state of each nitrogen atom in diazene is -1 because each hydrogen atom has an oxidation state of +1 and the overall charge of the molecule is 0.
06

(f) Sodium Nitrate

Sodium nitrate has the chemical formula NaNO₃. In this compound, one sodium atom (oxidation state +1) is bonded to a nitrate ion (NO₃⁻). The nitrate ion (NO₃⁻) consists of one nitrogen atom and three oxygen atoms (each with an oxidation state of -2). The oxidation state of nitrogen in sodium nitrate is +5 because the total charge of the nitrate ion is -1, and the nitrogen atom balances the charges of the surrounding oxygen atoms.
07

(g) Nitrogen Trifluoride

Nitrogen trifluoride has the chemical formula NF₃. In this molecule, one nitrogen atom is bonded to three fluorine atoms, each of which has an oxidation state of -1. The oxidation state of nitrogen in nitrogen trifluoride is +3 because the total charge of the molecule is 0 and the nitrogen atom balances the charges of the surrounding fluorine atoms.
08

(h) Nitric Acid

Nitric acid has the chemical formula HNO₃. In this molecule, the nitrogen atom is bonded to one hydrogen atom (oxidation state +1) and three oxygen atoms (each with an oxidation state of -2). The oxidation state of nitrogen in nitric acid is +5 because the total charge of the molecule is 0, and the nitrogen atom balances the charges of the surrounding atoms.

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Most popular questions from this chapter

Nitric acid is a powerful oxidizing agent. Using standard reduction potentials, predict whether the following metals can be oxidized to +2 ions by nitric acid: (a) iron, (b) copper, (c) rhodium, (d) zinc, (e) lead, (f) tin.

Write a balanced equation for the reaction of each of the following compounds with water: (a) \(\mathrm{PCl}_{5}(s),\) (b) \(\mathrm{CO}_{2}(g)\) (c) \(\mathrm{K}_{2} \mathrm{O}_{2}(s)\) (d) \(\mathrm{Mg}_{3} \mathrm{P}_{2}(s)\) (e) \(\operatorname{LiAlH}_{4}(s)\) (f) \(\mathrm{Cl}_{2} \mathrm{O}(g)\) (g) \(\mathrm{NO}_{2}(g)\)

Identify each of the following elements as a metal, nonmetal, or metalloid: (a) boron, (b) barium, (c) argon, (d) caesium, (e) yttrium, (f) astatine.

Write a balanced equation for each of the following reactions: (a) Hydrogen cyanide is formed commercially by passing a mixture of methane, ammonia, and air over a catalyst at \(800^{\circ} \mathrm{C}\). Water is a by-product of the reaction. (b) Baking soda reacts with acids to produce carbon dioxide gas. (c) When barium carbonate reacts in air with sulfur dioxide, barium sulfate and carbon dioxide form.

Write a balanced equation for each of the following reactions: (a) Sulfur dioxide reacts with water. (b) Solid zinc sulfide reacts with hydrochloric acid. (c) Elemental sulfur reacts with sulfite ion to form thiosulfate. (d) Sulfur trioxide is dissolved in sulfuric acid.
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