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Chapter 22: Problem 56

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
The chemical formulas and nitrogen oxidation states for each compound are: (a) Nitric Oxide: NO, \(+2\) (b) Hydrazine: N2H4, \(-2\) (c) Potassium Cyanide: KCN, \(-3\) (d) Sodium Nitrite: NaNO2, \(+3\) (e) Ammonium Chloride: NH4Cl, \(-3\) (f) Lithium Nitride: Li3N, \(-3\)

Step by step solution

01

(a) Nitric Oxide

To find the chemical formula for nitric oxide, we first look for the common ions NO consists of: nitrogen (N), and oxygen (O). The formula for nitric oxide is NO, with 1 nitrogen atom and 1 oxygen atom. The oxidation state of nitrogen is +2 in this compound, following the rule that oxygen will typically have a -2 oxidation state.
02

(b) Hydrazine

Hydrazine is mainly constituted of nitrogen (N) and hydrogen (H) atoms. The chemical formula for hydrazine is N2H4, consisting of 2 nitrogen atoms and 4 hydrogen atoms. In this compound, the oxidation state of nitrogen is -2, as each hydrogen atom has an oxidation state of +1 (H has a +1 oxidation state when bonded to a non-metal, such as nitrogen).
03

(c) Potassium Cyanide

Potassium cyanide is composed of potassium (K) and a cyanide ion (CN^-). The chemical formula for potassium cyanide is KCN, with one potassium ion and one cyanide ion. In the cyanide ion, the nitrogen atom has an oxidation state of -3 due to the triple bond with carbon (with an oxidation state of +2).
04

(d) Sodium Nitrite

Sodium nitrite is made of sodium (Na) and a nitrite ion (NO2^-). The chemical formula for sodium nitrite is NaNO2, which includes one sodium ion and one nitrite ion. In the nitrite ion, nitrogen has an oxidation state of +3, as the two oxygen atoms each have an oxidation state of -2 (total -4), and the nitrogen atom must balance the overall charge to -1.
05

(e) Ammonium Chloride

Ammonium chloride contains an ammonium ion (NH4^+) and a chloride ion (Cl^-). The chemical formula for ammonium chloride is NH4Cl. In the ammonium ion, the nitrogen atom has an oxidation state of -3, which can be determined by knowing that each of the four hydrogen atoms has a +1 oxidation state, giving a total +4 charge for the ion, and Nitrogen must balance the overall charge to +1.
06

(f) Lithium Nitride

Lithium nitride is made up of lithium (Li) and nitrogen (N). The chemical formula for lithium nitride is Li3N, with three lithium ions and one nitrogen ion. In this compound, the oxidation state of the nitrogen atom is -3, as each of the three lithium atoms has a +1 oxidation state, and the nitrogen atom must balance the overall charge to zero.

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Most popular questions from this chapter

Hydrazine has been employed as a reducing agent for metals. Using standard reduction potentials, predict whether the following metals can be reduced to the metallic state by hydrazine under standard conditions in acidic solution: (a) \(\mathrm{Fe}^{2+},(\mathrm{b}) \mathrm{Sn}^{2+},(\mathrm{c}) \mathrm{Cu}^{2+}\), (d) \(\mathrm{Ag}^{+},(\mathrm{e}) \mathrm{Cr}^{3+}\).

Complete and balance the following equations: (a) \(\mathrm{CaO}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{Al}_{2} \mathrm{O}_{3}(s)+\mathrm{H}^{+}(a q) \longrightarrow\) (c) \(\mathrm{Na}_{2} \mathrm{O}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (d) \(\mathrm{N}_{2} \mathrm{O}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (e) \(\mathrm{KO}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (f) \(\mathrm{NO}(\mathrm{g})+\mathrm{O}_{3}(\mathrm{~g}) \longrightarrow\)

Manganese silicide has the empirical formula \(\mathrm{MnSi}\) and melts at \(1280^{\circ} \mathrm{C}\). It is insoluble in water but does dissolve in aqueous HF. (a) What type of compound do you expect MnSi to be, in terms of Table \(11.7 ?\) (b) Write a likely balanced chemical equation for the reaction of MnSi with concentrated aqueous HF.

Account for the following observations: (a) \(\mathrm{H}_{3} \mathrm{PO}_{3}\) is a diprotic acid. (b) Nitric acid is a strong acid, whereas phosphoric acid is weak. (c) Phosphate rock is ineffective as a phosphate fertilizer. (d) Phosphorus does not exist at room temperature as diatomic molecules, but nitrogen does. (e) Solutions of \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) are quite basic.

Write the Lewis structure for each of the following species, and describe its geometry: (a) \(\mathrm{NH}_{4}{ }^{+}\), (b) \(\mathrm{NO}_{2}^{-}\), (c) \(\mathrm{N}_{2} \mathrm{O}\), (d) \(\mathrm{NO}_{2}\).
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