Elements of period 3

A period 3 element is that chemical element in the third row (or period) of the periodic table.

The periodic table is arranged in rows to illustrate recurring (periodic) trends in the chemical behavior of elements as their atomic number increases: a new row is started when the periodic table skips a row and a chemical behavior begins to change. repeat, which means that elements with similar behavior fall into the same vertical columns. The third period contains eight elements: sodium, magnesium, aluminum, silicon, phosphorus, sulfur, chlorine, and argon. The first two, sodium and magnesium, are members of the s block of the periodic table, while the others are members of the p block of the Periodic Table. All period 3 elements occur in nature and have at least one stable isotope.

These are:

Elements of the period 1 - Elements of the period 2 - Elements of the period 3 - Elements of the period 4 - Elements of the period 5 - Elements of the period 6 - Elements of the period 7

Features

• They have the same number of orbitals.
• Atoms can house up to 5 subnives in the elements of period 3, which are:

1. 1 2
2. 22
3. 2p6
4. 32
5. 3p6

• And three levels that are:

K, L and M.

Elements

Sodium

Sodium (symbol Na) is a soft, silvery-white, highly reactive metal and is a member of the alkali metals; its only stable isotope is ²³Na. It is an abundant element that exists in numerous minerals such as feldspar, sodalite, and rock salt. Many sodium salts are highly soluble in water and are therefore present in significant quantities in Earth's bodies of water, most abundantly in the oceans as sodium chloride.

Many sodium compounds are useful, such as sodium hydroxide (lye) for soap making and sodium chloride for use as a de-icing agent and nutrient. The same ion is also a component of many minerals, such as sodium nitrate.

The free metal, elemental sodium, does not occur naturally, but must be prepared from sodium compounds. Elemental sodium was first isolated by Humphry Davy in 1807 by electrolysis of sodium hydroxide.

Magnesium

Magnesium (symbol Mg) is an alkaline earth metal and has a common oxidation number +2. It is the eighth most abundant element in the Earth's crust and ninth in the known universe as a whole. Magnesium is the fourth most common element on Earth as a whole (behind iron, oxygen and silicon), and makes up 13% of the planet's mass and a large fraction of the planet's mantle. It is relatively abundant because it is easily accumulated in supernova stars by sequential additions of three helium nuclei to carbon (which itself is made up of three helium nuclei). Due to its high content of magnesium ions and its solubility in water, it is the third most abundant element dissolved in seawater.

The free element (metal) does not occur naturally on Earth, as it is highly reactive (although once produced, it is coated with a thin layer of oxide [see passivation], which partly masks this reactivity). The free metal burns with a characteristic bright white light, making it a useful ingredient in sparklers. The metal is now obtained mainly by electrolysis of magnesium salts obtained from brine. Commercially, the primary use of the metal is as an alloying agent to make aluminum-magnesium alloys, sometimes called " magnalium " or "magnelium". Since magnesium is less dense than aluminum, these alloys are prized for their relative lightness and strength.

Magnesium ions are acidic to taste and, in low concentrations, help impart a natural acidity to fresh mineral waters.

Aluminum

Aluminum (symbol Al) is a silvery-white member of the boron group of chemical elements and a p-block metal classified by some chemists as a post-transition metal. It is not soluble in water under normal circumstances. Aluminum is the third most abundant element (after oxygen and silicon), and the most abundant metal, in the Earth's crust. It constitutes approximately 8% by weight of the solid surface of the Earth. Metallic aluminum is too chemically reactive to be produced natively. Instead, it is found combined in more than 270 different minerals. The main aluminum ore is bauxite.

Aluminum stands out for the low density of the metal and for its ability to resist corrosion due to the phenomenon of passivation. Structural components made of aluminum and its alloys are vital to the aerospace industry and are important in other areas of transportation and structural materials. The most useful aluminum compounds, at least by weight, are the oxides and sulfates.

Silicon

Silicon (symbol Si) is a group 14 metalloid. It is less reactive than its chemical analogue carbon, the nonmetal directly above it on the periodic table, but more reactive than germanium, the metalloid directly below it In the table. Controversy over the character of silicon dates from its discovery: silicon was first prepared and characterized in pure form in 1824, and was given the name silicon (Latin: silicis, flint)., with a -ium word ending to suggest a metal. However, its final name, suggested in 1831, reflects the chemically more similar elements carbon and boron.

Silicon is the eighth most common element in the universe by mass, but very rarely occurs as the pure free element in nature. It is most widely distributed in dust, sand, planetoids, and planets as various forms of silicon dioxide (silica) or silicates. More than 90% of the Earth's crust is composed of silicate minerals, making silicon the second most abundant element in the Earth's crust (about 28% by mass) after oxygen.

Most silicon is used commercially without being separated and, in fact, often with little processing from compounds from nature. These include the direct use of clays, silica sand, and stone in industrial buildings. Silica is used in ceramic bricks. Silicate goes into Portland cement for mortar and stucco, and is combined with silica sand and gravel to make concrete. Silicates are also found in porcelain-white ceramics and traditional quartz-based soda-lime glass. Newer silicon compounds such as abrasives in the form of silicon carbide and high-strength ceramics. Silicon is the basis for the ubiquitous silicon-based synthetic polymers called silicones.

Elemental silicon also has a major impact on the modern world economy. Although most of the free silicon is used in the steel refining, aluminum smelting, and fine chemical industries (often to make fumed silica), the relatively small portion of very highly purified silicon that is used in semiconductor electronics (<10%) is perhaps uniform. more critical. Due to the wide use of silicon in integrated circuits, the basis of most computers, much of modern technology depends on it.

Phosphorus

Phosphorus (symbol P) is a multivalent nonmetal of the nitrogen group, phosphorus as a mineral is almost always present in its maximum oxidation state (pentavalent), as inorganic phosphate rocks. Elemental phosphorus exists in two main forms, white phosphorus and red phosphorus, but due to its high reactivity, phosphorus is never found as a free element on Earth.

The first form of elemental phosphorus to be produced (white phosphorus, in 1669) emits a faint glow when exposed to oxygen; hence its name from Greek mythology, Φωσφόρος which means "bearer of light" (Lucifer in Latin), referring to the " Morning Star ", the planet Venus. Although the term " Phosphorescence ", meaning glow after illumination, is derived from this property of phosphor, phosphor glow is caused by oxidation of white (but not red) phosphor and should be called chemiluminescence. It is also the lightest element for easily producing stable exceptions to the octet rule.

The vast majority of phosphorus compounds are consumed as fertilizers. Other applications include the role of organophosphorus compounds in detergents, pesticides and nerve agents, and matches.

Sulfur

Sulfur (symbol S) is an abundant multivalent nonmetal, one of the chalcogens. Under normal conditions, sulfur atoms form cyclic octatomic molecules with chemical formula S₈. Elemental sulfur is a bright yellow crystalline solid when at room temperature. Chemically, sulfur can react as an oxidant or as a reducing agent. It oxidizes most metals and several nonmetals, including carbon, leading to its negative charge in most organosulfur compounds but reduces several strong oxidants, such as oxygen and fluorine.

In nature, sulfur can be found as a pure element and as sulfides and sulfate minerals. Mineral collectors often seek out elemental sulfur crystals for their brightly colored polyhedron shapes. Being abundant in a native form, sulfur was known in ancient times, mentioned for its uses in ancient Greece, China, and Egypt. Sulfur vapors were used as fumigants, and sulfur-containing medicinal mixtures were used as balms and antiparasitics. Sulfur was considered important enough to receive its own alchemical symbol. It was needed to make the best quality of black powder, and alchemists hypothesized that the bright yellow powder contained some of the properties of gold, which they sought to synthesize from it. In 1777, Antoine Lavoisier helped convince the scientific community that sulfur was a basic element, rather than a compound.

Elemental sulfur was once extracted from salt domes where it is sometimes found in nearly pure form, but this method has been obsolete since the turn of the century XX. Today, almost all elemental sulfur is produced as a byproduct of removing sulfur-containing contaminants from natural gas and oil. Commercial uses of the element are primarily in fertilizers, due to the relatively high requirement by plants, and in the manufacture of sulfuric acid, a primary industrial chemical. Other known uses of the element are in matches, insecticides, and fungicides. Many sulfur compounds are odorous and flavored natural gas, skunk, grapefruit, and garlic odors are due to sulfur compounds. Hydrogen sulfide produced by living organisms imparts the characteristic odor to rotten eggs and other biological processes.

Chlorine

Chlorine (symbol Cl) is the second lightest halogen. The element forms diatomic molecules under standard conditions, called dichloro. It has the highest electron affinity and the third highest electronegativity of all the elements; therefore, chlorine is a strong oxidizing agent.

The most common chlorine compound, sodium chloride (table salt), has been known since ancient times; however, around 1630, the Belgian chemist and physician Jan Baptist van Helmont obtained gaseous chlorine. The synthesis and characterization of elemental chlorine occurred in 1774 by the Swedish chemist Carl Wilhelm Scheele, who called it "dephlogistised muriatic acid air", since he thought that it synthesized the oxide obtained from hydrochloric acid because it was thought at that time that acids necessarily contained oxygen. Several chemists, including Claude Berthollet, suggested that "dephlogisticated muriatic acid air" de Scheele must be a combination of oxygen and the as yet undiscovered element. The suggestion that this newly discovered gas was a simple element was made in 1809 by Joseph Louis Gay-Lussac and Louis-Jacques. This was confirmed in 1810 by Sir Humphry Davy, who named it chlorine, from the Greek word χλωρός (chlōros), meaning "green-yellow".

Chlorine is a component of many other compounds. It is the second most abundant halogen and the twenty-first most abundant chemical element in the Earth's crust. The great oxidizing power of chlorine led to its bleaching and disinfectant uses, as well as being an essential reagent in the chemical industry. As a common disinfectant, chlorine compounds are used in swimming pools to keep them clean and sanitary. In the upper atmosphere, chlorine-containing molecules, such as chlorofluorocarbons, have been implicated in ozone depletion.

Argon

Argon (symbol Ar) is the third element of group 18, the noble gases. Argon is the third most common gas in Earth's atmosphere at 0.93%, making it more common than carbon dioxide. Almost all of this argon is radiogenic argon-40 derived from the decay of potassium-40 in the earth's crust. In-universe, argon-36 is by far the most common argon isotope, being the preferred argon isotope produced by stellar nucleosynthesis.

The name "argon" is derived from the Greek neuter adjective ἀργόν meaning "lazy" or "the inactive one", since the element undergoes almost no chemical reactions. The full octet (eight electrons) in the outer atomic shell makes argon stable and resistant to bonding with other elements. Its triple point temperature of 83.8058 K is a defining fixed point on the 1990 International Temperature Scale.

Argon is produced industrially by fractional distillation of liquid air. Argon is used primarily as an inert shielding gas in welding and other high-temperature industrial processes in which normally unreactive substances become reactive: for example, an argon atmosphere is used in electric graphite furnaces to prevent the graphite to burn Argon gas also has uses in incandescent and fluorescent lighting, and other types of gas discharge tubes. The argon produces a distinctive blue-green gas laser.