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Chapter 22: Problem 54

What is the oxidation state of sulfur in the following compounds? (a) \(\mathrm{S}_{2} \mathrm{Br}_{2}\) (b) \(\mathrm{SCl}_{2}\) (c) \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\) (d) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}_{4} \mathrm{O}_{6}\).

Short Answer

Expert verified
The oxidation states of sulfur in the compounds are (a) +1, (b) +2, (c) +2, and (d) +5.

Step by step solution

01

Calculation for \( \mathrm{S}_{2} \mathrm{Br}_{2} \)

Given that bromine is usually -1 in compounds and since the compound is neutral, the total of all oxidation states should be zero. Therefore, we assign bromine an oxidation state of -1 and find sulfur's oxidation number by subtracting the total oxidation state of bromine from zero. This gives us that the oxidation state of sulfur is +1.
02

Calculation for \(\mathrm{SCl}_{2}\)

The total oxidation state of a neutral molecule must be zero. Given that chlorine usually has an oxidation number of -1 in compounds, this means that the sulfur must have an oxidation state of +2.
03

Calculation for \(\mathrm{Na}_{2} \mathrm{S}_{2} \mathrm{O}_{3}\)

Sodium is always +1, and oxygen is usually -2. This means each sulfur atom must have an oxidation state of +2 to achieve overall neutrality.
04

Calculation for \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}_{4} \mathrm{O}_{6}\)

The ammonium cation, \( \mathrm{NH}_{4}^{+} \), always has a charge of +1. Oxygen usually has an oxidation number of -2. Thus, considering the total charge in the molecule to be zero, the sulfur atoms must have an oxidation number of +5.

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Most popular questions from this chapter

Use VSEPR theory to predict the probable geometric structures of the molecules (a) \(\mathrm{O}_{2} \mathrm{XeF}_{2} ;\) (b) \(\mathrm{O}_{3} \mathrm{XeF}_{2}\) (c) OXeF \(_{4}\).

What volume of \(\mathrm{H}_{2}(\mathrm{g})\) at \(25^{\circ} \mathrm{C}\) and \(752 \mathrm{mmHg}\) is required to hydrogenate oleic acid, \(\mathrm{C}_{17} \mathrm{H}_{33} \mathrm{COOH}(1)\) to produce one mole of stearic acid, \(\mathrm{C}_{17} \mathrm{H}_{35} \mathrm{COOH}(\mathrm{s}) ?\) Assume reaction (22.52) proceeds with a 95\% yield.

All of the following compounds yield \(\mathrm{O}_{2}(\mathrm{g})\) when heated to about \(1000 \mathrm{K}\) except (a) \(\mathrm{KClO}_{3} ;\) (b) \(\mathrm{KClO}_{4}\) (c) \(\mathrm{N}_{2} \mathrm{O} ;\) (d) \(\mathrm{CaCO}_{3} ;\) (e) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\).

The boiling points of oxygen and argon are \(-183^{\circ} \mathrm{C}\) and \(-189^{\circ} \mathrm{C},\) respectively. Because the boiling points are so similar, argon obtained from the fractional distillation of liquid air is contaminated with oxygen. The following three-step procedure can be used to obtain pure argon from the oxygen-contaminated sample: (1) Excess hydrogen is added to the mixture and then the mixture is ignited. (2) The mixture from step (1) is then passed over hot copper(II) oxide. (3) The mixture from step (2) is passed over a dehydrated zeolite material (see Chapter 21 ). Explain the purpose of each step, writing chemical equations for any reactions that occur.

Write a chemical equation for the hydrolysis of \(\mathrm{XeF}_{4}\) that yields \(\mathrm{XeO}_{3}, \mathrm{Xe}, \mathrm{O}_{2},\) and \(\mathrm{HF}\) as products.
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