Oxygen Compounds: Definition, Examples and List

Oxygen is one essential constituent of life on Earth; it has its applications running from the biological to the chemical processes. In reality, when we breathe, oxygen is used by the body to create energy within our system. It, however, doesn't stop there; it forms different compounds of importance in everyday life and industrially as well. Everything from the glass of water we drink to most of the materials that we use consists of compounds of oxygen. We will thus learn about these compounds of oxygen in this article, their meanings, types, and applications in various aspects of life. Description of important compounds such as oxides, peroxides, and superoxides will be done in detail regarding the method of formation, properties, and uses. By the end, you will have in-depth knowledge of what these compounds are and why they are important to your academic learning and practical life.

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This Story also Contains

1. Various Aspects and Types of Oxygen Compounds
2. Properties
3. Uses
4. Significance and Applications in Real Life and Academics
5. Some Solved Examples
6. Summary

Major Concept: Definitions and Descriptions
Compounds of oxygen represent a class of chemical substances that contain atoms of oxygen linked to another element. The best known are oxides, in which oxygen has been combined with some other element. For instance, the reaction of oxygen with metals leads to metal oxides, a good example being iron oxide, more commonly known as rust. They also occur in non-metal oxides, an example being carbon dioxide, a very vital component in the earth's carbon cycle. Several bonds may be formed with one element, thus giving rise to a variety of oxides that have different properties. Besides oxide, some other volatile oxygen compounds are peroxides—which have the anion O2 —, and an oxygen–oxygen single bond—, and superoxides, which have an oxygen–oxygen bond with extra electrons and hence are very reactive. From these basic definitions flow a good deal of the enormous and diverse world of oxygen compounds.

Various Aspects and Types of Oxygen Compounds

It must therefore be broadly classified into oxides, peroxides, and superoxides. It shows different characteristics and applications in these groups. Oxides are the most common and they occur in both natural surroundings and constructed environments. Examples include silicon dioxide, commonly sand, and aluminum oxide, used on abrasives. Peroxides are less stable and mostly utilized in bleaching and disinfecting agents; hydrogen peroxide is a strong example that is very familiar to most people. The highly reactive superoxides are normally used in specialized applications such as chemical oxygen generators in submarines and spacecraft. Another important category includes the hydroxides, where oxygen is bonded to hydrogen and another element, forming compounds like sodium hydroxide, commonly known as lye or caustic soda, which has quite wide application in cleaning stuff. All these different kinds of oxygen compounds have varying properties that set them to be put into various uses, hence pointing out their versatility and their importance.

Preparation
Dioxygen can be obtained in the laboratory in the following ways:

• By heating oxygen-containing salts such as chlorates, nitrates, and permanganates.$2 \mathrm{KClO}_3 \xrightarrow[\mathrm{MnO}_2]{\text { Heat }} 2 \mathrm{KCl}+3 \mathrm{O}_2$
• By the thermal decomposition of the oxides of metals low in the electrochemical series and higher oxides of some metals.$\begin{aligned} & 2 \mathrm{Ag}_2 \mathrm{O}(\mathrm{s}) \rightarrow 4 \mathrm{Ag}(\mathrm{s})+\mathrm{O}_2(\mathrm{~g}) \\ & 2 \mathrm{HgO}(\mathrm{s}) \rightarrow 2 \mathrm{Hg}(\mathrm{l})+\mathrm{O}_2(\mathrm{~g})\end{aligned}$
• Hydrogen peroxide is readily decomposed into water and dioxygen by catalysts such as finely divided metals and manganese dioxide.
  $2 \mathrm{H}_2 \mathrm{O}_2(\mathrm{aq}) \rightarrow 2 \mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{O}_2(\mathrm{~g})$
  On a large scale, it can be prepared from water or air. Electrolysis of water leads to the release of hydrogen at the cathode and oxygen at the anode.

Properties

Dioxygen is a colorless and odorless gas. Its solubility in water is to the extent of 3.08 cm³ in 100 cm³ water at 293 K which is just sufficient for the vital support of marine and aquatic life. It liquefies at 90 K and freezes at 55 K. The Oxygen atom has three stable isotopes: ¹⁶O, ¹⁷O, and ¹⁸O. Molecular oxygen, O₂ is unique in being paramagnetic despite having an even number of electrons. Dioxygen directly reacts with nearly all metals and non-metals except some metals ( e.g., Au, Pt) and some noble gases. Its combination with other elements is often strongly exothermic which helps in sustaining the reaction. However, to initiate the reaction, some external heating is required as the bond dissociation enthalpy of the oxygen-oxygen double bond is high (493.4 kJ mol^–1).

Uses

• It is used in oxyacetylene welding.
• In the manufacture of many metals, particularly steel.
• Oxygen cylinders are widely used in hospitals, high-altitude flying, and in mountaineering.
• The combustion of fuels, e.g., hydrazines in liquid oxygen, provides tremendous thrust in rockets.

Significance and Applications in Real Life and Academics

The oxygen compounds hold a significant place in many everyday life issues and academics as well. The following details each, in turn: We encounter oxygen compounds in our daily lives all the time: water, H₂O, which is essential to all known forms of life; carbon dioxide, CO₂, which is exhaled by animals and used for photosynthesis by plants. Oxides are of immense importance to industries. For example, silicon dioxide is used when manufacturing electronics and making glass. For instance, hydrogen peroxide is a peroxide used for bleaching and disinfecting. In environmental studies, knowledge of the behavior of oxides is applied to NOx and SOx, examples of oxides that are key causes and factors of climate change. Chemically, it helps in understanding chemical bonding and reactivity and principles of oxidation-reduction reactions, being of the core nature in chemistry education. These compounds' applications also mirror the importance associated with oxygen compounds in a wide range of critical areas, such as health, environment and industry, and academia.

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Some Solved Examples

Example 1
Question: The Brown's gas is
1. used in oxy-hydrogen welding
2. used as an oxygen mask
3. used in the refrigerator
4. None

Solution: As we have learned, Brown's gas is used in oxy-hydrogen welding. Hence, the correct answer is option (1).

Example 2
Question: Select the correct statement about $( O_2 )$ gas:
1. It is stable in nature
2. It is neutral in nature
3. It is used as a bleaching agent
4. All the above are correct

Solution: As we have learned, dioxygen gas is stable, neutral, and has bleaching action. Hence, the correct answer is option (4).

Example 3
Question: Which of the following is used as rocket fuel?
1. liquid He
2. liquid $( Cl_2 )$
3. liquid $( O_2 )$
4. liquid U

Solution: As we have learned, liquid $( O_2 )$ is used as rocket fuel. Hence, the correct answer is option (3).

Summary

The compounds of oxygen, whether as oxides, peroxides, or superoxides, play a very significant role in nature and human applications. These compounds form an integral part and center of life, industry, and environmental science; thus, the chemistry of oxygen compounds assumes a central place in the study of chemistry. Their origins of formation, properties, and applications explain why they are so pervasive and vital in our lives—from the water we drink to the air that we breathe and commodities used by us, oxygen is always there compounded. On the other hand, from these different forms and uses, we realize manifold their versatility and importance in practical and academic contexts alike.