Occurrence, Preparation, and Properties of Sulfur, Representative Metals, Metalloids, and Nonmetals | Chemistry 2e

Learning objectives

By the end of this section, you will be able to:

Describe the properties, preparation, and uses of sulfur

Sulfur exists in nature as elemental deposits as well as sulfides of iron, zinc, lead, and copper, and sulfates of sodium, calcium, barium, and magnesium. Hydrogen sulfide is often a component of natural gas and occurs in many volcanic gases, like those shown in CNX_Chem_18_10_Volcano. Sulfur is a constituent of many proteins and is essential for life.

View original figure (external; image not reproduced in this text edition)

Original figure description: A lake is shown surrounded by rocky, mountainous peaks. A white vapor rises from the ground near the lake.

Volcanic gases contain hydrogen sulfide. (credit: Daniel Julie/Wikimedia Commons)

The Frasch process, illustrated in CNX_Chem_18_10_FrachMine, is important in the mining of free sulfur from enormous underground deposits in Texas and Louisiana. Superheated water (170 °C and 10 atm pressure) is forced down the outermost of three concentric pipes to the underground deposit. The hot water melts the sulfur. The innermost pipe conducts compressed air into the liquid sulfur. The air forces the liquid sulfur, mixed with air, to flow up through the outlet pipe. Transferring the mixture to large settling vats allows the solid sulfur to separate upon cooling. This sulfur is 99.5% to 99.9% pure and requires no purification for most uses.

View original figure (external; image not reproduced in this text edition)

Original figure description: A diagram is shown in which a vertical tube is embedded on the lower end into a multilayered solid. The upper layer is labeled, “Soil,” and the lower layer is labeled, “Solid sulfur deposit.” A thin tube, beginning at the top of the diagram, leads into the vertical tube to the bottom and is labeled, “Compressed air.” Left-facing and then down-facing arrows are drawn on this inner tube. These arrows then turn upward at the bottom of the tube and are drawn upward to indicate the flow of, “Liquid sulfur,” from the bottom of the diagram to the top outside the inner tube. These arrows lead to a chamber at the top right of the diagram with arrows facing to the left labeled, “Sulfur, water and air.” A horizontal tube in the center right of the diagram leads to the outer tube and arrows drawn downward lead back to the bottom of the diagram. This tube is labeled, “Superheated water.”

The Frasch process is used to mine sulfur from underground deposits.

Larger amounts of sulfur also come from hydrogen sulfide recovered during the purification of natural gas.

Sulfur exists in several allotropic forms. The stable form at room temperature contains eight-membered rings, and so the true formula is S₈. However, chemists commonly use S to simplify the coefficients in chemical equations; we will follow this practice in this book.

Like oxygen, which is also a member of group 16, sulfur exhibits a distinctly nonmetallic behavior. It oxidizes metals, giving a variety of binary sulfides in which sulfur exhibits a negative oxidation state (2−). Elemental sulfur oxidizes less electronegative nonmetals, and more electronegative nonmetals, such as oxygen and the halogens, will oxidize it. Other strong oxidizing agents also oxidize sulfur. For example, concentrated nitric acid oxidizes sulfur to the sulfate ion, with the concurrent formation of nitrogen(IV) oxide:

S (s) + 6 {HNO}_{3} (a q) ⟶ 2 H_{3} O^{+} (a q) + {SO}_{4} 2− (a q) + 6 {NO}_{2} (g)

The chemistry of sulfur with an oxidation state of 2− is similar to that of oxygen. Unlike oxygen, however, sulfur forms many compounds in which it exhibits positive oxidation states.

Key Concepts and Summary

Sulfur (group 16) reacts with almost all metals and readily forms the sulfide ion, S²⁻, in which it has as oxidation state of 2−. Sulfur reacts with most nonmetals.

Chemistry End of Chapter Exercises

Explain why hydrogen sulfide is a gas at room temperature, whereas water, which has a lower molecular mass, is a liquid.

Give the hybridization and oxidation state for sulfur in SO₂, in SO₃, and in H₂SO₄.

SO₂, sp² 4+; SO₃, sp², 6+; H₂SO₄, sp³, 6+

Which is the stronger acid, NaHSO₃ or NaHSO₄?

Determine the oxidation state of sulfur in SF₆, SO₂F₂, and KHS.

SF₆: S = 6+; SO₂F₂: S = 6+; KHS: S = 2−

Which is a stronger acid, sulfurous acid or sulfuric acid? Why?

Oxygen forms double bonds in O₂, but sulfur forms single bonds in S₈. Why?

Sulfur is able to form double bonds only at high temperatures (substantially endothermic conditions), which is not the case for oxygen.

Give the Lewis structure of each of the following:

(a) SF₄

(b) K₂SO₄

(d) H₂SO₃

(e) SO₃

Write two balanced chemical equations in which sulfuric acid acts as an oxidizing agent.

There are many possible answers including: $Cu (s) + 2 H_{2} {SO}_{4} (l) ⟶ {CuSO}_{4} (a q) + {SO}_{2} (g) + 2 H_{2} O (l)$ and $C (s) + 2 H_{2} {SO}_{4} (l) ⟶ {CO}_{2} (g) + 2 {SO}_{2} (g) + 2 H_{2} O (l)$

Explain why sulfuric acid, H₂SO₄, which is a covalent molecule, dissolves in water and produces a solution that contains ions.

How many grams of Epsom salts (MgSO₄⋅7H₂O) will form from 5.0 kg of magnesium?

5.1 $\times$ 10⁴ g

Glossary

Frasch process: important in the mining of free sulfur from enormous underground deposits

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