Double Bubble Map for Oxygen and Sulfur

Double Bubble Map for Oxygen and Sulfur

Oxygen

Oxygen is by far the most abundant element in Earth’s crust, constituting about 46 percent of its mass. In addition, the atmosphere contains about 21 percent molecular oxygen by volume (23 percent by mass). Like nitrogen, oxygen in the free state is a diatomic molecule (O2). In the laboratory, oxygen gas can be obtained by heating potassium chlorate.

2KClO3(s) > 2KCl(s) + 3O2(g)

The reaction is usually catalyzed by manganese(IV) dioxide, MnO2. Pure oxygen gas can be prepared by electrolyzing water. Industrially, oxygen gas is prepared by the fractional distillation of liquefied air. Oxygen gas is colorless and odorless. Oxygen is a building block of practically all biomolecules, accounting for about a fourth of the atoms in living matter. Molecular oxygen is the essential oxidant in the metabolic breakdown of food molecules. Without it, a human being cannot survive for more than a few minutes.

Properties of Diatomic Oxygen

Although oxygen has two allotropes, O2 and O3, when we speak of molecular oxygen, we normally mean O2. Ozone, O3, is less stable than O2. The O2 molecule is paramagnetic because it contains two unpaired electrons.

A strong oxidizing agent, molecular oxygen is one of the most widely used industrial chemicals. Its main uses are in the steel industry and in sewage treatment. Oxygen is also used as a bleaching agent for pulp and paper, in medicine to ease breathing diffi culties, in oxyacetylene torches, and as an oxidizing agent in many inorganic and organic reactions.

Oxides, Peroxides, and Superoxides

Oxygen forms three types of oxides: the normal oxide (or simply the oxide), which contains the O22 ion; the peroxide, which contains the O^2— ion; and the superoxide, which contains the O₂^2— ion:

The ions are all strong Brønsted bases and react with water as follows:

Oxide: O₂^2— (aq) + H2O(l) > 2OH^—(aq)

Peroxide: 2O₂^2— (aq) + 2H2O(l) > O2(g) + 4OH2(aq)

Superoxide: 4O₂^2— (aq) + 2H2O(l) > 3O2(g) + 4OH2(aq)

Note that the reaction of O^2— with water is a hydrolysis reaction, but those involving

O₂^2—and O₂^— are redox processes.

The nature of bonding in oxides changes across any period in the periodic table. Oxides of elements on the left side of the periodic table, such as those of the alkali metals and alkaline earth metals, are generally ionic solids with high melting points. Oxides of the metalloids and of the metallic elements toward the middle of the periodic table are also solids, but they have much less ionic character. Oxides of nonmetals are covalent compounds that generally exist as liquids or gases at room temperature. The acidic character of the oxides increases from left to right.

Properties of Oxygen

Oxygen is odorless, tasteless and colorless. In liquid and solid form, oxygen is pale blue and is a strong paramagnetic.

Oxygen Use

Oxygen in the form of elements and compounds widely used in everyday life.

1)     Oxygen Gas

Oxygen gas is used in the processing of iron into open open steel (oxygen furnace). Oxygen in the form of oxyethethylene (a mixture of carbide and oxygen gas) is used to clean the crust and refine the bulges in the steel product. In addition oxygen also plays a role in the burning of metals, pengobatab in hospitals and industrial waste aeration.

2)    Ozone

The ozone layer contains a layer of Earth's atmosphere as a protective UV radiation. In industry, Ozone is used as a bleach and killer agent of microorganisms. The bottled drinking water industry also disinfects its products using this ozone compound.

Sulfur

Although sulfur is not a very abundant element (it constitutes only about 0.06 percent of Earth’s crust by mass), it is readily available because it occurs commonly in nature in the elemental form. The largest known reserves of sulfur are found in sedimentary deposits. In addition, sulfur occurs widely in gypsum (CaSO4.2H2O) and various sulfide minerals such as pyrite (FeS2). Sulfur is also present in natural gas as H2S, SO2, and other sulfur-containing compounds.

Sulfur is extracted from underground deposits by the Frasch process. In this process, superheated water (liquid water heated to about 160°C under high pressure to prevent it from boiling) is pumped down the outermost pipe to melt the sulfur. Next, compressed air is forced down the innermost pipe. Liquid sulfur mixed with air forms an emulsion that is less dense than water and therefore rises to the surface as it is forced up the middle pipe. Sulfur produced in this manner, which amounts to about 10 million tons per year, has a purity of about 99.5 percent.

Sulfur Characteristics

Sulfur is pale yellow, a fragile solid, which is insoluble in water but easily soluble in CS2 (carbon disulphide). In various forms, whether gaseous, liquid or solid, sulfuric elements occur with more than one or allotropeous allotropes. With different forms, consequently the nature is different and the relationship between the nature and form of allotropnya still can not be understood.

This substance has unusual electrical and optical properties. Sulfur with a purity of 99.999 +% is commercially available.

Amorphous sulfur or plastic sulfur is obtained by quenching crystals suddenly and rapidly. X-ray studies show that amorphous sulfur has a helical structure with eight atoms on each spiral. The sulfur crystals are thought to consist of a ring shape with eight sulfur atoms, which are mutually reinforcing giving a normal X-ray pattern.

Sulfur Use

Sulfur is a component of gunpowder and is used in the process of vulcanization of natural rubber and also acts as a fungicide (SO2). Sulfur is used heavily in the manufacture of phosphate fertilizers. Tons of sulfur are used to produce sulfuric acid, which is a very important chemical.

Sulfur is also used for the manufacture of sulphite paper and other paper, to sterilize the smoker, and to bleach the dried fruit. Sulfur is a good insultor.

Sulfur is very important for life. Sulfur is a constituent of fat, body fluids and bone mineral, in a small degree.

Sulfur quickly removes odors.

Sodium thiosulfate pentahydrate (Na2SO4.5H2O) is used as a film washer. This compound is known as the hypo peacock.

Sulfuric acid (H2SO4) is used as solvent, battery charger, salt making, fertilizer manufacture, oil treatment, and textile dyeing.