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Chapter 3: Problem 64

Write a formula for (a) an oxide of nitrogen with \(\mathrm{N}\) in the O.S. \(+5 ;\) (b) an oxoacid of nitrogen with \(\mathrm{N}\) in the O.S. \(+3 ;\) (c) an oxide of carbon in which the apparent O.S. of \(C\) is \(+4 / 3 ;\) (d) a sulfur- containing oxoanion in which the apparent O.S. of \(S\) is +2.5 and the ionic charge is \(2-\).

Short Answer

Expert verified
The formula for: (a) an oxide of nitrogen is \(N_2O_5\); (b) an oxoacid of nitrogen is \(HNO_2\); (c) an oxide of carbon is \(C_3O_4\); (d) a sulfur-containing oxoanion is \(H_2S_2O_5^{2-}\).

Step by step solution

01

Determining the formula for an oxide of nitrogen

In an oxide of nitrogen where Nitrogen has an oxidation state (O.S) of +5, Nitrogen is bound to Oxygen which typically has an oxidation state of -2. In order for the total compound to be neutral, Nitrogen’s positive charge must be neutralized by Oxygen’s negative charge. Therefore, one Nitrogen atom with a +5 oxidation state will bind with 2.5 or, in whole numbers, 5 Oxygen atoms with a -2 oxidation state each. Therefore, the formula for the oxide will be \(N_2O_5\).
02

Writing formula for an oxoacid of nitrogen

An oxoacid typically contains Hydrogen, Oxygen and another element. The other element in this case is Nitrogen which has an oxidation state of \(+3\), Oxygen has an oxidation state of \(-2\), and Hydrogen has an oxidation state of \(+1\). To keep the total charge neutral, 3 Hydrogen's can neutralize the -3 charge from Oxygen, and one Nitrogen with +3 charge can neutralize the remaining charge. So the formula for the oxoacid of Nitrogen will be \(HNO_2\).
03

Determining the formula for an oxide of Carbon

In this case, Carbon has an oxidation state of \(+4/3\), which implies that to maintain charge balance with Oxygen (-2 oxidation state), three Carbon atoms are required against four Oxygen atoms. Therefore, the formula for the oxide of Carbon will be \(C_3O_4\).
04

Writing the formula for a sulfur-containing oxoanion

In this case, Sulfur has an oxidation state of \(+2.5\) and the ionic charge is \(2-\). Therefore, to maintain the charge balance with Oxygen having an oxidation state of \(-2\), two Sulfur atoms are required against five Oxygen atoms. And, to neutralize the ionic charge, we need two Hydrogen atoms. Therefore, the formula for the sulfur-containing oxoanion will be \(H_2S_2O_5^{-2}\).

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Most popular questions from this chapter

Without doing detailed calculations, explain which of the following has the greatest mass percent of sulfur. $\mathrm{SO}_{2}, \mathrm{S}_{2} \mathrm{Cl}_{2}, \mathrm{Na}_{2} \mathrm{S}, \mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}, \mathrm{or} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{SH}$

Explain each term as it applies to the element nitrogen. (a) atomic mass; (b) molecular mass; (c) molar mass.

Anhydrous sodium sulfate, \(\mathrm{Na}_{2} \mathrm{SO}_{4},\) absorbs water vapor and is converted to the decahydrate, \(\mathrm{Na}_{2} \mathrm{SO}_{4} \cdot 10 \mathrm{H}_{2} \mathrm{O} .\) How much would the mass of \(24.05 \mathrm{g}\) of anhydrous \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) increase if converted completely to the decahydrate?

Name the following compounds and specify which ones are best described as ionic: (a) \(\mathrm{OF}_{2} ;\) (b) \(\mathrm{XeF}_{2}\) (c) \(\operatorname{CuSO}_{3} ;\) (d) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\)

A public water supply was found to contain 1 part per billion (ppb) by mass of chloroform, \(\mathrm{CHCl}_{3}\) (a) How many \(\mathrm{CHCl}_{3}\) molecules would be present in a \(225 \mathrm{mL}\) glass of this water? (b) If the \(\mathrm{CHCl}_{3}\) in part (a) could be isolated, would this quantity be detectable on an ordinary analytical balance that measures mass with a precision of ±0.0001 g?
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