Question

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

Examples of sulfur compounds with various oxidation states are: 1. For an oxidation state of +6, sulfuric acid (H₂SO₄) is an example. 2. For an oxidation state of +4, sulfur dioxide (SO₂) is an example. 3. For an oxidation state of +2, hydrogen sulfide (H₂S) is an example. 4. For an oxidation state of 0, elemental sulfur (S) is an example. 5. For an oxidation state of -2, a sulfide ion (S²⁻) found in compounds like iron sulfide (FeS) is an example.

Step-by-step solution

Oxidation state: +6

One example of a sulfur compound with an oxidation state of +6 is sulfuric acid (H₂SO₄). In this compound, sulfur is bonded to four oxygen atoms and has an overall charge of +6.

Oxidation state: +4

An example of a sulfur compound with an oxidation state of +4 is sulfur dioxide (SO₂). In this compound, sulfur is bonded to two oxygen atoms and has an overall charge of +4.

Oxidation state: +2

One example of a sulfur compound with an oxidation state of +2 is hydrogen sulfide (H₂S). In this compound, sulfur is bonded to two hydrogen atoms and has an overall charge of +2.

Oxidation state: 0

An example of a sulfur compound with an oxidation state of 0 is elemental sulfur (S). In its elemental form, sulfur is not bonded to any other atoms and thus has an oxidation state of 0.

Oxidation state: -2

One example of a sulfur compound with an oxidation state of -2 is a sulfide ion (S²⁻), which can be found in compounds like iron sulfide (FeS). In this case, sulfur has an overall charge of -2 as it gains two electrons from the metal atom it is bonded to.

Key concepts

Sulfur Compounds

Sulfur is an intriguing element because it forms several different compounds, displaying a variety of oxidation states. Let's explore them step by step:

• In nature, sulfur compounds play vital roles, such as in the formation of minerals and as essential elements in biological systems.
• Sulfur compounds are frequently involved in industrial processes. This includes the production of fertilizers or the synthesis of chemicals.
• Each sulfur compound has unique properties, influencing its chemical reactivity and usage.

Understanding sulfur compounds starts with recognizing the oxidation states sulfur can exhibit in these compounds, which we'll explore in the next sections.

Oxidation States Chemistry

Oxidation states in chemistry tell us about the loss or gain of electrons by an element in a compound. Sulfur showcases a notable variety, exhibiting +6, +4, +2, 0, and -2 states. Here's how these states work:

• The oxidation state helps in understanding the electron configuration and distribution in sulfur compounds.
• They are crucial for determining how sulfur will react with other elements, such as oxygen or metals.
• The numerical value reflects net electron loss (positive values) or gain (negative values).

This concept forms a foundation for discussing specific sulfur compounds, like sulfuric acid, where sulfur takes a particular oxidation state.

Sulfuric Acid

Sulfuric acid (\(\text{H}_2\text{SO}_4\)) is a key sulfur compound where sulfur is in its +6 oxidation state. What makes sulfuric acid so significant?

• It is one of the most industrially important chemicals, widely used to manufacture fertilizers, dyes, and detergents.
• Sulfur in sulfuric acid achieves a +6 oxidation state by "losing" electrons to oxygen through its strong covalent bonds.
• The acid has two hydrogen atoms covalently bonded, contributing to its strong acidic properties.

The understanding of sulfuric acid's chemistry highlights the importance of sulfur's highest oxidation state.

Sulfur Dioxide

In sulfur dioxide (\(\text{SO}_2\)), sulfur occupies a +4 oxidation state. This compound is particularly important due to its environmental impact as well as its uses.

• It is a significant component of air pollution, known for its role in acid rain formation.
• Industrially, sulfur dioxide is used in the production of sulfuric acid and as a preservative in food and wine.
• Sulfur forms two double bonds with oxygen, explaining its +4 oxidation state due to the gain of partial electron density.

The chemistry of sulfur dioxide serves as a reminder of the intricate balance required in industrial processes and environmental health.

Elemental Sulfur

Elemental sulfur, denoted simply as \(\text{S}\), exhibits an oxidation state of 0. In nature, elemental sulfur is found in its purest form and has distinct properties:

• Appearing commonly as a bright yellow powder or crystalline solid, elemental sulfur does not have bonds altering its electron configuration.
• It is relatively stable, not readily reacting under ordinary conditions.
• Elemental sulfur is essential in vulcanization processes in the rubber industry and in the production of sulfur dioxide through combustion.

Understanding elemental sulfur's oxidation states sheds light on its wide range of uses and stability.