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Chapter 20: Problem 63

Sulfur forms a wide variety of compounds in which it has \(+6\), \(+4,+2,0\), and \(-2\) oxidation states. Give examples of sulfur compounds having each of these oxidation states.

Short Answer

Expert verified
Examples of sulfur compounds with different oxidation states are: 1. Sulfuric acid (H₂SO₄), where sulfur has an oxidation state of +6. 2. Sulfur dioxide (SO₂), where sulfur has an oxidation state of +4. 3. Hydrogen sulfite (HSO₃⁻), where sulfur has an oxidation state of +2. 4. Elemental sulfur (S₈), where sulfur has an oxidation state of 0. 5. Hydrogen sulfide (H₂S), where sulfur has an oxidation state of -2.

Step by step solution

01

Example of Sulfur with an Oxidation State of +6

One example of a sulfur compound with an oxidation state of +6 is sulfuric acid (H₂SO₄). In this molecular structure, the sulfur atom is bonded to four oxygen atoms and has a double bond with two of them. This results in a total oxidation state of +6 because the sulfur atom loses 6 electrons in these bonds.
02

Example of Sulfur with an Oxidation State of +4

A compound where sulfur has an oxidation state of +4 is sulfur dioxide (SO₂). In this molecule, the sulfur atom forms a double bond with two oxygen atoms. Each double bond results in an oxidation state of +2, which adds up to a total oxidation state of +4 for sulfur.
03

Example of Sulfur with an Oxidation State of +2

An example of a sulfur compound with an oxidation state of +2 is hydrogen sulfite (HSO₃⁻). In this ion, the sulfur atom is bonded to three oxygen atoms and has a double bond with one of them. The resulting oxidation state for the sulfur atom is +2, as it loses 2 electrons in the bond formation.
04

Example of Sulfur with an Oxidation State of 0

Sulfur in its elemental form, sulfur (S₈), has an oxidation state of 0. This molecule consists of 8 sulfur atoms connected in a ring, and since all the atoms are the same element, there is no transfer of electrons in the bond formation, leaving the oxidation state of each sulfur atom at 0.
05

Example of Sulfur with an Oxidation State of -2

The most common example of a sulfur compound with an oxidation state of -2 is hydrogen sulfide (H₂S). In this molecule, sulfur forms single covalent bonds with two hydrogen atoms. Since sulfur is more electronegative than hydrogen, it gains one electron from each hydrogen atom, resulting in a -2 oxidation state for the sulfur atom.

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Most popular questions from this chapter

Discuss the importance of the \(\mathrm{C}-\mathrm{C}\) and \(\mathrm{Si}-\mathrm{Si}\) bond strengths and of \(\pi\) bonding to the properties of carbon and silicon.

List two major industrial uses of hydrogen.

The heaviest member of the alkaline earth metals is radium (Ra), a naturally radioactive element discovered by Pierre and Marie Curie in \(1898 .\) Radium was initially isolated from the uranium ore pitchblende, in which it is present as approximately \(1.0 \mathrm{~g}\) per \(7.0\) metric tons of pitchblende. How many atoms of radium can be isolated from \(1.75 \times 10^{8} \mathrm{~g}\) pitchblende \((1\) metric ton \(=\) \(1000 \mathrm{~kg}) ?\) One of the early uses of radium was as an additive to paint so that watch dials coated with this paint would glow in the dark. The longest-lived isotope of radium has a half-life of \(1.60 \times 10^{3}\) years. If an antique watch, manufactured in 1925, contains \(15.0 \mathrm{mg}\) radium, how many atoms of radium will remain in \(2025 ?\)

Write a balanced equation describing the reduction of \(\mathrm{H}_{2} \mathrm{SeO}_{4}\) by \(\mathrm{SO}_{2}\) to produce selenium.

Hydrazine is somewhat toxic. Use the following half-reactions to explain why household bleach (highly alkaline solution of sodium hypochlorite) should not be mixed with household ammonia or glass cleansers that contain ammonia. \(\mathrm{ClO}^{-}+\mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{OH}^{-}+\mathrm{Cl}^{-} \quad \mathscr{E}^{\circ}=0.90 \mathrm{~V}\) \(\mathrm{N}_{2} \mathrm{H}_{4}+2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{NH}_{3}+2 \mathrm{OH}^{-} \quad \mathscr{E}^{\circ}=-0.10 \mathrm{~V}\)
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