Question

Match the following Column-I (a) Peroxide (b) Superoxide (c) Dioxide (d) Suboxide Column-II (p) \(\mathrm{C}_{3} \mathrm{O}_{2}\) (q) \(\mathrm{PbO}_{2}\) (r) \(\mathrm{KO}_{2}\) (s) \(\mathrm{H}_{2} \mathrm{O}_{2}\) (t) \(\mathrm{RbO}_{2}\)

Short answer

(a) - (s), (b) - (r), (b) - (t), (c) - (q), (d) - (p)

Step-by-step solution

Understanding the Concept of Peroxides

Peroxides are compounds that contain an oxygen-oxygen single bond. The general structure can be represented as ext{R-O-O-R'}, where \( R \) is any organic or inorganic group. These compounds release oxygen when decomposed. A common example of a peroxide is \( \text{H}_2\text{O}_2 \), hydrogen peroxide.

Identifying the Superoxide

Superoxides are compounds that contain the superoxide ion \( \text{O}_2^- \). These ions have an extra electron compared to the peroxide ion. Alkali metal superoxides such as \( \text{KO}_2 \) and \( \text{RbO}_2 \) are common and are recognized by their oxygen-rich composition.

Recognizing Dioxide Compounds

Dioxides are made up of one element chemically bonded to two oxygen atoms. An example is lead dioxide, \( \text{PbO}_2 \), which is a typical dioxide compound.

Identifying the Suboxide

Suboxides are less common and less oxygen-rich compared to other oxides. An example of a suboxide is \( \text{C}_3\text{O}_2 \), where carbon-to-oxygen ratio is less than the traditional oxides.

Matching Column-I to Column-II

Now we match each item in Column-I to Column-II based on the definitions: - (a) Peroxide matches with (s) \( \text{H}_2\text{O}_2 \) because it's a classic example of a peroxide. - (b) Superoxide matches with (r) \( \text{KO}_2 \) and (t) \( \text{RbO}_2 \) since both are characterized as superoxides containing \( \text{O}_2^- \). - (c) Dioxide matches with (q) \( \text{PbO}_2 \) since it follows the formula of dioxides with two oxygen atoms.- (d) Suboxide matches with (p) \( \text{C}_3\text{O}_2 \) because it fits as a suboxide with fewer oxygens.

Key concepts

Peroxide Compounds

Peroxide compounds are unique due to their distinctive chemical structure, featuring an oxygen-oxygen single bond. This bond is often depicted as \( \text{R-O-O-R'} \), where \( R \) can stand for various organic or inorganic groups. A distinctive quality of peroxides is their ability to release oxygen, especially when decomposed under certain conditions.

Hydrogen peroxide, denoted as \( \text{H}_2\text{O}_2 \), is perhaps the most familiar example. In everyday uses, it's often employed for its bleaching and disinfecting properties. Its ability to decompose and release oxygen makes it a powerful cleaning agent.

Other examples include peroxide ion-containing compounds such as sodium peroxide (\( \text{Na}_2\text{O}_2 \)), often used in chemical reactions that necessitate oxidizing conditions.

Superoxide Ions

Superoxide ions are recognized for their additional electron, giving them the formula \( \text{O}_2^- \). This extra electron imparts unique reactivity to superoxides, making them highly powerful oxidizing agents.

Commonly seen in alkali metal compounds such as potassium superoxide (\( \text{KO}_2 \)) and rubidium superoxide (\( \text{RbO}_2 \)), superoxides play an essential role in various chemical and biological processes. For instance, they are used in life support and rebreathing apparatuses. Here, they serve a crucial function by releasing oxygen as they react with carbon dioxide from exhaled air, forming carbonate.

Such properties not only underline their practical applications but also their potential hazards, as they can be quite reactive. Proper handling and understanding of their chemistry is essential.

Dioxide Chemistry

Dioxide compounds are characterized by the presence of two oxygen atoms bonded to one other element. Lead dioxide (\( \text{PbO}_2 \)) is a classic example, often employed in industrial applications such as in lead-acid batteries.

Diodes’ stable bonding structure provides a range of functional characteristics. They often serve as oxidizing agents, facilitating many chemical reactions by donating oxygen atoms. Lead dioxide, specifically, is used in the electrodes of car batteries, playing a vital role in generating electric power.

Moreover, the dioxide structure is essential in natural processes and synthetic chemistry, contributing to environmental processes like photosynthesis and cellular respiration.

Suboxide Characteristics

Suboxides are less commonly encountered in chemistry compared to other oxide types. They are distinguished by having a lower ratio of oxygen relative to the other element involved. A well-known example is trimethylene dioxide (\( \text{C}_3\text{O}_2 \)) with a carbon-to-oxygen ratio that is lower than in typical oxides.

This gives suboxides certain unique properties, including distinctive electronic configurations and structures. While not as prevalent or widely studied as other oxides, suboxides nevertheless hold potential for niche applications and intrigue in theoretical chemistry for their atypical bonding and reaction patterns.

As always, the understanding of these compounds is fundamental to expanding materials science and the development of new technologies.