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 the specified oxidation states are as follows: 1. +6 oxidation state: Sulfuric acid (H2SO4) 2. +4 oxidation state: Sulfur dioxide (SO2) 3. +2 oxidation state: Hydrogen sulfite ion (HSO3^-) 4. 0 oxidation state: Elemental sulfur (S8) 5. -2 oxidation state: Hydrogen sulfide (H2S)

Step-by-step solution

Example of Sulfur in +6 Oxidation State

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

Example of Sulfur in +4 Oxidation State

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

Example of Sulfur in +2 Oxidation State

One example of a sulfur compound with a +2 oxidation state is hydrogen sulfite ion (HSO3^-). In this ion, sulfur is bonded to three oxygen atoms and one hydrogen atom. The sulfur atom has an oxidation state of +2.

Example of Sulfur in 0 Oxidation State

One example of a sulfur compound with a 0 oxidation state is elemental sulfur (S8). In this compound, sulfur exists as a ring of eight sulfur atoms where each sulfur atom is bonded to two other sulfur atoms. The sulfur atoms have an oxidation state of 0.

Example of Sulfur in -2 Oxidation State

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

Key concepts

Sulfur Compounds

Sulfur compounds are a diverse group of chemical substances that contain sulfur atoms in different oxidation states. Sulfur can exhibit several oxidation states, including

• +6 (as in sulfuric acid)
• +4 (as in sulfur dioxide)
• +2 (as in hydrogen sulfite)
• 0 (as in elemental sulfur)
• -2 (as in hydrogen sulfide)

These various states allow sulfur to form a wide array of compounds, each with unique properties and uses.
Sulfur compounds are vital in both industrial processes and biological functions. They are found in many natural sources, including volcanic emissions and mineral deposits. Understanding the oxidation states of sulfur in these compounds is crucial as it helps predict their reactivity and stability.

Sulfur-containing compounds play essential roles in processes such as the manufacturing of fertilizers, pharmaceuticals, and rubber. Furthermore, they are significant in environmental chemistry, especially related to air pollution through sulfur dioxide and hydrogen sulfide emissions.

Sulfuric Acid

Sulfuric acid (\[H_2SO_4\] ) is one of the most well-known sulfur compounds, featuring sulfur in a +6 oxidation state. It's a strong acid, commonly used in industry for

• Fertilizer production
• Refining petroleum
• Numerous chemical synthesis reactions

Due to its highly corrosive nature, it must be handled with care.
The sulfur atom in sulfuric acid is centrally located with four oxygen atoms arranged around it. This structure allows it to act as both an oxidizing and a dehydrating agent.

Sulfuric acid is also vital in domestic and commercial cleaning products. Its strong acidity makes it effective for removing rust and scaling. Despite its wide use and importance, safety precautions and guidelines are critical to follow to prevent its hazardous effects.

Elemental Sulfur

Elemental sulfur is sulfur in its pure form, often found as octasulfur (\[S_8\]), where it exhibits a 0 oxidation state. In this form, sulfur molecules create a ring composed of eight sulfur atoms.
This gives it a unique yellow color and allows it to exist as a solid at room temperature. Elemental sulfur is commonly obtained from natural sources such as

• Volcanic emissions
• Sulfide mineral deposits

and through industrial extraction methods.

It is used extensively in agriculture for making fertilizers and pesticides. Elemental sulfur is also a critical component in the vulcanization of rubber, providing elasticity and durability in rubber products.
Moreover, it is used in the manufacture of sulfuric acid and as a fungicide in vineyards. Its diverse applications illustrate its significance across various industrial and agricultural sectors.

Hydrogen Sulfide

Hydrogen sulfide (\[H_2S\] ) features sulfur in a -2 oxidation state, bonded with two hydrogen atoms. Known for its distinct rotten egg smell, hydrogen sulfide gas is highly toxic and flammable. It naturally occurs in

• Sewage systems
• Hot springs
• Volcanic gases

Hydrogen sulfide is produced by the bacterial breakdown of organic matter in the absence of oxygen, a process known as anaerobic digestion.

In industry, hydrogen sulfide can serve as a precursor to elemental sulfur. The gas is also crucial in laboratory processes, primarily when producing metal sulfides for materials and electronics.
Handling hydrogen sulfide requires strict safety measures due to its potential health hazards. Its presence in both natural and industrial contexts underscores the need for proper monitoring and management to ensure safety.