oxygen group element
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What are oxygen group elements?
The oxygen group elements, also known as Group 16 or VIa, are a set of six chemical elements in the periodic table: oxygen (O), sulfur (S), selenium (Se), tellurium (Te), polonium (Po), and livermorium (Lv).
These elements have six electrons in their outermost shell, leading to a tendency to gain two more electrons to form stable, doubly negative charged ions. This property, typical of nonmetallic elements, is expressed through electronegativity and electron affinity. Oxygen stands out with the highest electronegativity and electron affinity, except for fluorine.
The lightest element in the group, oxygen, exhibits unique properties compared to the other elements due to its small atomic size and electronic structure.
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Which elements belong to the oxygen group?
The oxygen group, also known as Group 16 (VIa) of the periodic table, consists of six chemical elements: oxygen (O), sulfur (S), selenium (Se), tellurium (Te), polonium (Po), and livermorium (Lv). Oxygen is a colorless, odorless, tasteless gas essential to living organisms. Sulfur exists as a pale yellow, crystalline, nonmetallic solid. Selenium is a nonmetal and is rarely found in its uncombined state. Tellurium is a silvery-white element with properties intermediate between those of metals and nonmetals. Polonium is a rare, radioactive element found in uranium-containing minerals. Livermorium is a synthetic element created in a particle accelerator.
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What are some common properties of oxygen group elements?
The oxygen group elements, found in Group 16 of the periodic table, share several common properties. Their electron configurations feature six electrons in the outermost shell, leading to a tendency to gain two more electrons to form stable, doubly negative charged ions.
Key properties include:
* Electronegativity and electron affinity These properties decrease as you move down the group.
* Oxidation states While oxygen typically exhibits a -2 oxidation state, heavier chalcogens favor positive states like +2 and +4. All elements in the group, except oxygen, can have positive oxidation states.
* Catenation This is the bonding of an atom to another identical atom. Sulfur is second only to carbon in exhibiting this property.
* Atomic size The sizes of atoms of elements vary regularly throughout the periodic system.
* Reactivity Oxygen is a very reactive element.5 Britannica SourcesCreated from Britannica articles using AI. AI can make mistakes, so verify using Britannica articles. -
Why is oxygen important in this group?
Oxygen is crucial within its group due to its high electronegativity and electron affinity, second only to fluorine. This enables oxygen to readily form negative ions by gaining electrons, defining it as an oxidizing agent.
As the lightest element in Group 16, oxygen's unique properties, such as its small atomic size, differentiate it from heavier chalcogens like sulfur. Unlike other elements in the group, oxygen strongly resists positive oxidation states.
Furthermore, oxygen is essential for life, utilized by animals and plants. It also forms compounds with almost every element. Though essential for life, molecular oxygen can be toxic and mutagenic.
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How do oxygen group elements react with other elements?
The oxygen group elements, also known as Group 16 or VIa, consist of oxygen (O), sulfur (S), selenium (Se), tellurium (Te), polonium (Po), and livermorium (Lv). These elements have six electrons in their outermost shell, leading them to form stable shells by gaining two electrons and creating a double negative charge.
Oxygen stands out with the highest electronegativity and electron affinity, except for fluorine. The tendency to gain electrons decreases as you move down the group, with tellurium and polonium behaving more like metals, tending to lose electrons. While polonium can exhibit a -2 oxidation state, heavier chalcogens favor positive states like +2 and +4. Except for oxygen, all can achieve positive oxidation states, with +6 being unstable for heavier members, causing them to revert to lower states or elemental form.
Sulfides, selenides, and tellurides are strong reducing agents, readily oxidized to their free elements. Oxygen typically bonds with two other atoms, as seen in water (H2O). The ability to catenate, or bond with identical atoms, is prominent in sulfur, second only to carbon.
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oxygen group element, any of the six chemical elements making up Group 16 (VIa) of the periodic classification—namely, oxygen (O), sulfur (S), selenium (Se), tellurium (Te), polonium (Po), and livermorium (Lv). A relationship between the first three members of the group was recognized as early as 1829; tellurium was assigned its place by 1865, and polonium was discovered in 1898. In 2000, Russian and American physicists created livermorium, the sixth member of Group 16, in a particle accelerator.
Natural occurrence and uses
Estimates of the proportions of the various kinds of atoms in the universe put oxygen fourth in abundance, after hydrogen, helium, and neon, but the importance of such a ranking is slight, since hydrogen atoms account for almost 94 percent of the total and helium for most of the rest. About three atoms out of 10,000 are oxygen, but because the mass of an oxygen atom is approximately 16 times that of a hydrogen atom, oxygen constitutes a larger fraction of the mass of the universe, though still only about 0.5 percent. In the regions ordinarily accessible to man, however—i.e., within a few kilometres of the surface of the Earth—oxygen is the most abundant element: in mass, it makes up about 20 percent of the air, about 46 percent of the solid crust of the Earth, and about 89 percent of the water.
Oxygen is represented by the chemical symbol O. In the air, oxygen exists mostly as molecules each made up of two atoms (O2), although small amounts of ozone (O3), in which three atoms of oxygen make up each molecule, are present in the atmosphere. Oxygen is a colourless, odourless, tasteless gas essential to living organisms, being taken up by animals, which convert it to carbon dioxide; plants, in turn, utilize carbon dioxide as a source of carbon and return the oxygen to the atmosphere. Oxygen forms compounds by reaction with practically any other element, as well as by reactions that displace elements from their combinations with each other; in many cases, these processes are accompanied by the evolution of heat and light and in such cases are called combustions.
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In cosmic abundance, sulfur ranks ninth among the elements, accounting for only one atom of every 20,000–30,000. Sulfur occurs in the uncombined state as well as in combination with other elements in rocks and minerals that are widely distributed, although it is classified among the minor constituents of the Earth’s crust, in which its proportion is estimated to be between 0.03 and 0.06 percent. On the basis of the finding that certain meteorites contain about 12 percent sulfur, it has been suggested that deeper layers of the Earth contain a much larger proportion. Seawater contains about 0.09 percent sulfur in the form of sulfate. The most important source is underground deposits of very pure sulfur present in domelike geologic structures where the sulfur is believed to have been formed by the action of bacteria upon the mineral anhydrite, in which sulfur is combined with oxygen and calcium. Deposits of sulfur in volcanic regions probably originated from gaseous hydrogen sulfide generated below the surface of the Earth and transformed into sulfur by reaction with the oxygen in the air.
Sulfur exists under ordinary conditions as a pale yellow, crystalline, nonmetallic solid; it is odourless and tasteless, combustible, and insoluble in water. Its chemical symbol is S. It reacts with all metals except gold and platinum, forming sulfides; it also forms compounds with several of the nonmetallic elements. Several million tons of sulfur are produced each year, mostly for the manufacture of sulfuric acid, which is widely used in industry.
The element selenium (symbol Se) is much rarer than oxygen or sulfur, comprising approximately 90 parts per billion of the crust of the Earth. It is occasionally found uncombined, accompanying native sulfur, but is more often found in combination with heavy metals (as copper, mercury, lead, or silver) in a few minerals. The principal commercial source of selenium is as a by-product of copper refining; its major uses are in the manufacture of electronic equipment, in pigments, and in making glass. The gray, metallic form of the element is the most stable under ordinary conditions; this form has the unusual property of greatly increasing in electrical conductivity when exposed to light. Selenium compounds are toxic to animals; plants grown in seleniferous soils may concentrate the element and become poisonous.
Tellurium is a silvery-white element (symbol Te) with properties intermediate between those of metals and nonmetals; it makes up approximately one part per billion of the Earth’s crust. Like selenium, it is less often found uncombined than as compounds of metals such as copper, lead, silver, or gold, and is obtained chiefly as a by-product of the refining of copper or lead. No large use for tellurium has been found.
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Polonium (symbol Po) is an extremely rare, radioactive element found in minerals containing uranium. It has some scientific applications as a source of alpha radiation.