Detailed First Twenty Periodic Elements

Fig. 1: Symbols, names, and atomic numbers for elements 1-20.

The first atomic element in the periodic table is hydrogen with the atomic number of 1 and an atomic symbol: H , an electron configuration of Hydrogen is the most abundant element . About 90% of the atoms and 75% of the element mass of the universe is hydrogen. Although hydrogen is the most abundant element in the human body in terms of numbers of atoms of the element, it's only 3rd in abundance by mass, after oxygen and carbon, because hydrogen is so light. Its Atomic Weight (1.00794) makes hydrogen the lightest element. It is so light, the pure element isn't bound by Earth's gravity. So, there is very little hydrogen gas left in the atmosphere. Massive planets, such as Jupiter, consist mainly of hydrogen, much like the Sun and stars. Even though hydrogen, as a pure element, bonds to itself to form H2, it's still lighter than a single atom of helium because most hydrogen atoms don't have any neutrons. In fact, two hydrogen atoms (1.008 atomic mass units per atom) are less than half the mass of one helium atom (atomic mass 4.003 Hydrogen is the one of the simplest and most commonly found chemical element making up about seventy five of its elemental mass and is found throughout the universe as ice , water on another habitable planet , giant gas planets or even the massive stars that use hydrogen in powering interstellar fusion and more than half our planet consist of water , in standard pressure conditions under room temperature hydrogen is odorless , tasteless and colorless There are three natural isotopes of hydrogen: protium, deuterium, and tritium. The most common isotope of hydrogen is protium, which has 1 proton, 0 nuetrons, and 1 electron. This makes hydrogen the only element that can have atoms without any neutrons! Deuterium has 1 proton, 1 neutron, and 1 electron. Although this isotope is heavier than protium, deuterium is not radioactive. However, tritium does emit radiation. Tritium is the isotope with 1 proton, 2 neutrons, and 1 electron. Hydrogen gas is extremely flammable. It is used as a fuel by the space shuttle main engine and was associated with the famous explosion of the Hindenburg airship. While many people consider oxygen to be flammable, it actually it doesn’t burn on its own however it's an oxidizer, which is why hydrogen is so explosive in air or with oxygen. Hydrogen compounds commonly are commonly called hydrides, Hydrogen may be produced by reacting metals with acids (e.g., zinc with hydrochloric acid). The physical form of hydrogen at room temperature and pressure is a colorless and odorless gas and the liquid is a nonmetal, but when hydrogen is compressed into a solid, the element is an alkali metal. Solid crystalline metallic hydrogen has the lowest density of any crystalline solid. Hydrogen has many uses, though most hydrogen is used for processing fossil fuels and in the production of ammonia. It is gaining importance as an alternate fuel that produces energy by combustion, similar to what happens in fossil fuel engines. Hydrogen is also used in fuel cells that react hydrogen and oxygen to produce water and electricity. In compounds, hydrogen can take a negative charge (H-) or a positive charge (H+). Hydrogen is the only atom for which the Schrödinger equation has an exact solution.

The second element of the atomic table is Helium which is a noble or inert gas that is lighter than air, it has an atomic symbol of He and an atomic number of 2, atomic weight 4.00 and an electron configuration of 1s2 seven isotopes of helium are known. Helium is a very light, inert, colorless and odorless gas. This gas has the lowest melting point of any known element and it is the only liquid that cannot be solidified by lowering the temperature, instead it remains a liquid down to absolute zero at ordinary pressures however it can be solidified by increasing the pressure. The specific heat of helium gas is unusually high as the density of helium vapor at the normal boiling point is also very high, with the vapor expanding greatly when heated up to room temperature. Although helium normally has a valence of zero, it has a weak tendency to combine with specific types of other elements. Helium is widely used in cryogenic research because its boiling point is near absolute zero (4.216 K degrees) melting point 0.95 K degrees.) It is used in the study of superconductivity, as an inert gas shield for arc welding, as a protective gas in growing silicon and germanium crystals and producing titanium and zirconium, for pressuring liquid fuel rockets, for use in magnetic resonance imaging (MRI), as a cooling medium in nuclear reactors, as a gas for supersonic wind tunnels, for instances a mixture of helium and oxygen is used as an artificial atmosphere for divers and others working under pressure. Helium is used for filling balloons and blimps, except for hydrogen because people can’t get over how hydrogen balloons exploded, helium is the most abundant element in the universe. It is an important component in the proton-proton reaction and the carbon cycle, which account for the energy of the sun and stars. Helium is extracted from natural gas. In fact, all natural gas contains at least trace quantities of helium. The fusion of hydrogen into helium is the sources of a hydrogen bomb's energy and due to this disintegration of the material of releasing its energy is a product of radioactive substances, so it is found in ores of uranium, radium, and other elements.

Lithium is the third and most abused element by humans used in futile power systems which explode it has an atomic symbol of Li, atomic number 3, atomic weight 6.93 and an electron configuration of [He]2s1 Lithium has a melting point of 180.54°C, boiling point of 1342°C, specific gravity of 0.534 (20°C), and a valence of 1. It is the lightest of the metals and has 8 isotopes [Li-4 to Li-11]. Li-6 (7.59% abundance) and Li-7 (92.41% abundance) are both stable. With a density approximately half that of water it is a soft, silvery-white alkali metal. Under ordinary conditions, lithium is the least dense of the solid elements. It has the highest specific heat of any solid element. Metallic Lithium is silvery in appearance. It reacts with water, but not as vigorously as does sodium. Lithium imparts a crimson color to flame, although the metal itself burns a bright white. Lithium is corrosive and requires special handling. Elemental lithium is extremely flammable. Lithium is used in heat transfer applications. It is used as an alloying agent, in synthesizing organic compounds, and is added to glasses and ceramics. Its high electrochemical potential makes it useful for battery anodes. Lithium chloride and lithium bromide are highly hygroscopic, so are used as drying agents. Lithium stearate is used as a high-temperature lubricant. Lithium has medical applications, as well. Lithium does not occur free in nature. It is found in small amounts in practically all igneous rocks and in the waters of mineral springs and is the only known alkali metal that reacts with nitrogen. The minerals that contain lithium include lepidolite, petalite, amblygonite, and spodumene. Lithium metal is produced electrolitically from the fused chloride. Lithium was first discovered in the mineral petalite (LiAlSi4O10) Lithium is used to create the hydrogen isotope tritium through bombardment of neutrons.

The fourth element is Beryllium having an atomic symbol of Be and an atomic number of 4 atomic weight 9.01 and electron configuration of [He]2s2 Beryllium has a melting point of 1287+/-5°C, boiling point of 2970°C, specific gravity of 1.848 (20°C), and valence of 2 Beryllium has ten known isotopes, ranging from Be-5 to Be-14. Be-9 is the only stable isotope. The metal is steel-gray in color, very light, with one of the highest melting points of the light metals. Its modulus of elasticity is a third higher than that of steel. Beryllium has high thermal conductivity, is nonmagnetic, and resists attack by concentrated nitric acid. Beryllium resists oxidation in air at ordinary temperatures. The metal has a high permeability to x-radiation. When bombarded by alpha particles, it yields neutrons in the ratio of approximately 30 million neutrons per million alpha particles. Beryllium and its compounds are toxic and should not be tasted to verify the metal's sweetness it is classified as an Alkaline-earth Metal. Precious forms of beryl include aquamarine, morganite, and emerald. Beryllium is used as an alloying agent in producing beryllium copper which is used for springs, electrical contacts, nonsparking tools, and spot-welding electrodes. It is used in many structural components of the space shuttle and other aerospace craft. Beryllium foil is used in x-ray lithography for making integrated circuits. It is used as a reflector or moderator in nuclear reactions. Beryllium is used in gyroscopes and computer parts. The oxide has a very high melting point and is used in ceramics and nuclear applications.
Beryllium is found in approximately 30 mineral species, including beryl (3BeO Al2O3·6SiO2), bertrandite (4BeO·2SiO2·H2O), chrysoberyl, and phenacite. The metal may be prepared by reducing beryllium fluoride with magnesium metal. Pure beryllium was isolated in 1828 by two different chemist independently: German chemist Friederich Wöhler and French chemist Antonie Bussy. Beryllium was originally named 'glyceynum' due to the sweet taste of beryllium salts. (glykis is Greek for 'sweet'). The name was changed to beryllium to avoid confusion with other sweet tasting elements and a genus of plants called glucine. Beryllium became the official name of the element in 1957.

James Chadwick bombarded beryllium with alpha particles and observed a subatomic particle with no electrical charge, leading to the discovery of the neutron. Wöhler was the chemist who first proposed the name beryllium for the new element.

boron which is the fifth element in the periodic table and has an atomic symbol of B with an atomic number of 5 atomic weight of 10.81 and electron configuration of [He]2s22p1 The melting point of boron is 2079°C, its boiling/sublimation point is at 2550°C, the specific gravity of crystalline boron is 2.34, the specific gravity of the amorphous form is 2.37, and its valence is 3. Natural boron is 19.78% boron-10 and 80.22% boron-11. B-10 and B-11 are the two stable isotopes of boron. Boron has a total of 11 known isotopes ranging from B-7 to B-17. Crystalline boron is hard, brittle, lustrous black and a semimetal, Amorphous boron is a brown powder. Boron has interesting optical properties. The boron mineral ulexite exhibits natural fiberoptic properties. Elemental boron transmits portions of infrared light. At room temperature, it is a poor electrical conductor, but it is a good conductor at high temperatures. Boron is capable of forming stable covalently bonded molecular networks. Boron filaments have high strength, yet are lightweight.The energy band gap of elemental boron is 1.50 to 1.56 eV, which is higher than that of silicon or germanium. Although elemental boron is not considered to be a poison, assimilation of boron compounds has a cumulative toxic effect. the element Boron has many different kinds of uses including silicon manufacturing where a silicon plate, rod or wafer is blasted with ions or hot gas in order to introduce impurities ( Boron is used as a dopant in semiconductor production to make p-type semiconductors. )The isotope B-10 is a neutron absorber and used in control rods and emergency shutdown systems of nuclear generators. Boron is a component of strong neodymium magnets (Nd2Fe14B magnets) Boron compounds are being evaluated for treating arthritis. Boron compounds are used to produce borosilicate glass. Boron nitride is extremely hard, behaves as an electrical insulator, yet conducts heat, and has lubricating properties similar to graphite. Amorphous boron provides a green color in pyrotechnic devices. Boron compounds, such as borax and boric acid, have many uses. Boron-10 is used as a control for nuclear reactors, to detect neutrons, and as a shield for nuclear radiation. Boron is added to glass to increase its resistance to heat shock. Most chemistry glassware is made from borosilicate glass. Boron is not found free in nature, although boron compounds have been known for thousands of years. Boron occurs as borates in borax and colemanite and as orthoboric acid in certain volcanic spring waters. The primary source of boron is the mineral rasorite, also called kernite, which is found in Californa's Mojave Desert. Borax deposits are also found in Turkey. High-purity crystalline boron may be obtained by vapor phase reduction of boron trichloride or boron tribromide with hydrogen on electrically heated filaments. Boron trioxide may be heated with magnesium powder to obtain impure or amorphous boron, which is a brownish-black powder. Boron is available commercially at purities of 99.9999%.

Carbon is the sixth element and is most abundant and essential to carbon based lifeforms having an atomic symbol of C, atomic number of 6, an atomic weight of 12.01, and an electron configuration of [He]2s22p2 .. Carbon is a nonmetal that can bond with itself and many other chemical elements, forming nearly ten million compounds Carbon Forms numerous and varied compounds with limitless applications. Many thousands of carbon compounds are integral to life processes. (Carbon has the highest melting/sublimation point of the elements on the periodic table, the melting point of diamond is ~3550°C, with the sublimation point of carbon around 3800°C.) Diamond is prized as a gemstone and is used for cutting, drilling, and as bearings. Graphite is used as a crucible for melting metals, in pencils, for rust protection, for lubrication, and as a moderator for slowing neutrons for atomic fission. Carbon is found free in nature in three allotropic forms: amorphous (lampblack, boneblack), graphite, and diamond. A fourth form, 'white' carbon, is thought to exist. Diamond is one of the hardest substances, with a high melting point and index of refraction. There are seven natural isotopes of carbon. In 1961 the International Union of Pure and Applied Chemistry adopted the isotope carbon-12 as the basis for atomic weights. Carbon compounds have limitless uses for example in its elemental form, diamond is a gemstone and used for drilling/cutting; graphite is used in pencils, as a lubricant, and to protect against rust; while charcoal is used to remove toxins, tastes, and odors. The isotope Carbon-14 is used in radiocarbon dating. Elemental carbon can take the form of one of the hardest substances (diamond) or one of the softest (graphite).

Nitrogen is the seventh element present of the periodic table and is a great oxidizer Nitrogen gas (N2) makes up 78.1% of the volume of the Earth’s air. Nitrogen gas is colorless, odorless, and relatively inert. Its atomic Symbol N atomic number 7 atomic weight 14.00 and electron configuration [He]2s22p3 Liquid Nitrogen is also a colorless and odorless gas, and is similar in appearance to water. There are two allotropic forms of solid nitrogen, a and b, with a transition between the two forms at -237° C. Nitrogen's melting point -209.86° C, boiling point is -195.8° C, density is 1.2506 g/l, specific gravity is 0.0808 (-195.8° C) for the liquid and 1.026 (-252° C) for the solid. Nitrogen compounds are found in foods, fertilizers, poisons, and explosives. Nitrogen gas is used as a blanketing medium during the production of electronic components. Nitrogen is also used in annealing stainless steels and other steel products. Liquid nitrogen is used as a refrigerant. Although nitrogen gas is fairly inert, soil bacteria can 'fix' nitrogen into a usable form, which plants and animals can then utilize. Nitrogen is a component of all proteins. Nitrogen is responsible for the orange-red, blue-green, blue-violet, and deep violet colors of the aurora. Nitrogen gas is obtained by liquefaction and fractional distillation from the atmosphere. Nitrogen gas also can be prepared by heating a water solution of ammonium nitrite (NH4NO3). Nitrogen is found in all living organisms. Ammonia (NH3), an important commercial nitrogen compound, is often the starting compound for many other nitrogen compounds. Ammonia may be produced using the Haber process.

The eighth element on the periodic table and being most important to sustaining the Oxidation Reduction reaction in all carbon based lifeforms and is commonly known as oxygen. Oxygen has the atomic number 8, atomic symbol O, atomic weight of 15.9994 and an Electron Configuration of [He]2s22p4 in short form, By mass, oxygen is the most abundant element in the Homo Eructus and all other forms of human evolution and it is also the most abundant element in the Earth's crust (about 47% by mass) and the third most common element in the Universe. As stars burn hydrogen and helium, oxygen becomes more abundant as it is shot out into space to from nebulas and other stars. This makes sense since most of the body consists of water or H2O in the chemical formula sense and almost all of the planet earth’s surface consists of 96.5% (71% in the land mass) in total as both water vapor and bodies of water. Oxygen accounts for 61-65% of the mass of the human body. Even though there are many more atoms of hydrogen in your body than oxygen, each oxygen atom is 16 times more massive than a hydrogen atom, it was discovered by Carl Wilhelm Scheele in 1773, but he did not publish his work immediately, so his credit is often given to Joseph Priestly in 1774. It’s essential in both Animals and plants, they require oxygen for Cellular Respiration to do the work necessary for photosynthesis, Calvin Cycle etc. Plant photosynthesis drives the oxygen cycle, maintaining it around 21% in air. While the gas is essential for life, too much of it can be toxic or lethal. Symptoms of oxygen poisoning include vision loss, coughing, muscle twitching, and seizures. Oxygen gas normally is the divalent molecule O2. Ozone, O3, is a different form of pure oxygen and is made by massive electrical discharges (Lightning strikes) in the atmosphere which produce O3, which is classified as ozone, and strengthen the ozone layer of the atmosphere ( Nine isotopes of oxygen are known and classified however Natural oxygen is a mixture of three isotopes.). Atomic oxygen, which is also known as "singlet oxygen" can occur in nature and does occasionally, although the ion readily bonds to other elements Singlet oxygen may be found in the upper atmosphere. A single atom of oxygen usually has an oxidation number of -2. At normal pressure, oxygen poisoning occurs when the gas exceeds 50%. Although oxygen gas is colorless, odorless and tasteless, the Liquid and solid forms of oxygen are pale blue. At lower temperatures and higher pressures, oxygen changes its appearance from a blue monoclinic crystals to orange, red, black, shades and even a metallic appearance, Oxygen supports combustion. However, it is not a true flammable gas, it is considered an oxidizer since bubbles of pure oxygen don't burn. Oxygen is paramagnetic meaning it is weakly attracted to a magnet but doesn't retain permanent magnetism. Excited oxygen is responsible for the bright red, green, and yellow-green colors of the aurora. It's the molecule of primary importance to all carbon based life and as well as generating bright and colorful auroras.

Fluorine being the ninth element on the periodic table it is mainly used as a deceptive toothpaste additive meaning it does more harm than good just use hydrogen peroxide and was first isolated by Henri Moissan and also made the world's first artificial diamond by applying pressure to charcoal it should also be noted that hydrofluoric acid dissolves glass. Before Henri Moissan success to isolating fluorine through the electrolysis process , George Gore actually managed to obtain fluorine through the same process first however Fluorine is also known as the most chemically reactive (and electronegative) element being the lightest halogen and only exists in an elemental form as a highly toxic pale yellow diatomic gas under room conditions and does not react vigorously with oxygen, helium , neon or argon and is one of the few elements that will form compounds with other nobles gases such as xenon , krypton and radon .

Now we see the first double digit element on the table called neon with is key in most fluorescent lighting and being the tenth element on the periodic table

The next element, number eleven is sodium an alkali metal which is very important to carbon based lifeforms atomic symbol Na, atomic weight 22.98, atomic number 11 with an electron configuration of [Ne]3s118 isotopes are known. Only two are naturally occurring. Sodium derives its name from the Medieval Latin 'sodanum' and the English name 'soda'. The element symbol, Na, was shortened from the Latin name 'Natrium'. Swedish chemist Berzelius was the first to use the symbol Na for sodium in his early periodic table Sodium does not usually appear in nature on its own, but its compounds have been used by people for centuries. Elemental Sodium was not discovered until 1808. Davy isolated sodium metal using electrolysis from caustic soda or sodium hydroxide (NaOH) Sodium is the 6th most abundant element in the Earth's crust, making up approximately 2.6% of the earth, air, and oceans Sodium is not found free in nature, but sodium compounds are common such as the occurrence of Sodium in many minerals, such as cryolite, soda niter, zeolite, amphibole, and sodalite. The most common compound is sodium chloride or salt. Sodium floats on water, which decomposes it to evolve hydrogen and form the hydroxide. Sodium may ignite spontaneously on water. It does not usually ignite in air at temperatures below 115°C Sodium is used in fireworks to make an intense yellow color. The color is sometimes so bright it overwhelms other colors in a firework. The D lines of sodium's spectrum account for the dominate yellow color of the Sun. The top three countries that produce sodium are China, United States and India. Sodium metal is mass produced by electrolysis of sodium chloride.

Magnesium is the twelfth element on the periodic table atomic symbol Mg atomic number 12 atomic weight 24.30 electron configuration of [Ne] 3s2 Magnesium has a melting point of 648.8°C, boiling point of 1090°C, specific gravity of 1.738 (20°C), and a valance of 2.Magnesium metal is light (one-third lighter than aluminum), silvery-white, and it is a relatively tough metal but it tarnishes slightly in air. Finely, divided up magnesium ignites upon given activation energy in the open air, burning with a bright white flame. Magnesium also has an application in pyrotechnic and incendiary devices. It is alloyed with other metals to make them lighter and more easily welded, with applications in the aerospace industry. Magnesium is added to many propellants. It is used as a reducing agent in the preparation of uranium and other metals that are purified from their salts, Magnesite is also used in refactories.
Magnesium hydroxide (milk of magnesia), sulfate (Epsom salts), chloride, and citrate are used in medicine. Organic magnesium compounds have many uses. Magnesium is essential for plant and animal nutrition. Chlorophyll is a magnesium-centered porphyrin. Magnesium is the 8th most abundant element in the earth's crust, While not found free in nature, it is available in minerals including magnesite and dolomite. The metal may be obtained or refined by the electrolysis process of fused magnesium chloride derived from brines and seawater.

Aluminum is another commonly found element used in a wide variety of stuff. Aluminums number thirteen on the table with an atomic number of 13, atomic weight 26.98 and an Atomic symbol of Al. The electron configuration of aluminum in short form: [Ne]3s23p1 and the Shell Structure (2 8 3) aluminum is the third most abundant resource in the Earth's crust and was once called the "Metal of Kings" because pure aluminum was more expensive to produce than gold until the Hall-Heroult process was discovered. The primary source of aluminum is the ore bauxite and the element alone is not magnetic instead called paramagnetic Aluminum the most widely used metal after iron however it requires a lot of energy to separate from its ore, Recycling it only requires only 5% of that energy to produce the same amount. Aluminum can be 'rusted' or oxidized by mercury. Rubies are aluminum oxide crystals where some aluminum atoms have been replaced by chromium atoms. The top three countries that mine aluminum ore are Guinea, Australia and Vietnam. Australia, China and Brazil lead the world in aluminum production. The IUPAC adopted the name aluminum in 1990 and in 1993 recognized aluminum as an acceptable option for the element's name. A piece of jewelry in the tomb of the 3rd Century Chinese general Chou-Chu has been found to contain 85% aluminum. Historians do not know how the ornament was produced. Aluminum is used in fireworks to make or produce sparks and white flames. Aluminum is a common component of sparklers. Adjuvant in vaccines (chemical that disrupts immune response however for profit reasons it is said to enhance the immune system it also causes muscles to contract and nerves to degenerate or die around the area so people have more reason to believe the poisonous crap is actually good for you) All forms of alum can cause irritation of the skin and mucous membranes. Breathing alum can cause lung damage. Aluminum also may attack lung tissue. Because it's a salt, eating massive amounts of alum can make you sick. Usually ingesting alum will make you vomit, but if you could keep it down, the alum could upset the ionic equilibrium in your bloodstream, just like overdosing on any other electrolyte. However, the primary concern with alum is long-term exposure to low levels of the chemical. Aluminum, from your diet or healthcare product, can cause degeneration of nervous system tissue. It is possible exposure to aluminum could lead to an increased risk of certain cancers, brain plaques or Alzheimer's disease, Autism and an increased risk of exposure to more lethal diseases by degeneration of the immune system but it’s a good way to deceive the population and get their immune system suppressed.

Silicon is the next fourteenth element on the periodic table being most important to standard computer systems and standard diodes, electronics, etc. atomic symbol Si atomic number 14 atomic weight 28.05 electron configuration of [Ne]3s23p2 the properties of silicon include The melting point of silicon is 1410°C, boiling point is 2355°C, specific gravity is 2.33 (25°C), with a valence of 4. There are known isotopes of silicon ranging from Si-22 to Si-44. There are three stable isotopes: Al-28, Al-29, Al-30.Silicon is a semi metal, Crystalline silicon has a metallic grayish color. Silicon is relatively inert, but it is attacked by dilute alkali and by halogens. Silicon transmits over 95% of all infrared wavelengths (1.3-6.7 mm). Silicon is one of the most widely used elements. Silicon is important to plant and animal life. Diatoms extract silica from water to build their cell walls Silica can be found in plant ashes and in the human skeleton the semimetal also plays an important role in being an ingredient in steel. Silicon carbide is an important abrasive and is used in lasers to produce coherent light at 456.0 nm. Silicon doped with gallium, arsenic, boron, etc. is used to produce transistors, solar cells, rectifiers, and other important solid-state electronic devices or p-n junctions within them.
Silicones range from liquids to hard solids and have many useful properties, including use as adhesives, sealants, and insulators. Sand and clay are used to make building materials Silica is an ingredient used in tempering glass, which has many useful mechanical, electrical, optical, and thermal properties since Silicon oxide crystals in the form of quartz are piezoelectric. The resonance frequency of quartz is used in many precision timepieces. Silicon crystals for electronics must have a purity of one billion atoms for every non-silicon atom (99.9999999% pure). Silicon makes up 25.7% of the earth's crust, by weight, making it the second most abundant element (exceeded by oxygen). Silicon can be found anywhere in the sun, stars and even a principal component of the class of meteorites known as aerolites. Silicon is also a component of tektites, a natural glass of uncertain origin. Silicon does not occur naturally instead it commonly occurs as the oxide and silicates, including sand, quartz, amethyst, agate, flint, jasper, opal citrine granite, hornblende, feldspar, mica, clay, and asbestos. Silicon may be prepared by heating silica and carbon in an electric furnace, using carbon electrodes. The amorphous form of silicon may be prepared as a brown powder, which can then be melted or vaporized. The Czochralski process is used to produce single crystals of silicon for solid-state and semiconductor devices. Hyperpure silicon may be prepared by a vacuum float zone process and by thermal decompositions of ultra-pure trichlorosilane in an atmosphere of hydrogen.

The fifteenth element present on the table is phosphorus a Non-Metal with the atomic classification of : atomic symbol P atomic number 15 atomic weight 30.97 electron configuration of [Ne] 3s2 3p3 The melting point of phosphorus (white) is 44.1°C, boiling point (white) is 280°C, specific gravity (white) is 1.82, (red) 2.20, (black) 2.25-2.69, with a valence of 3 or 5. There are four allotropic forms of phosphorus: two forms of white (or yellow), red, and black (or violet). White phosphorus exhibits a and b modifications, with a transition temperature between the two forms at -3.8°C. Ordinary phosphorus is a waxy white solid, Phosphorus has 22 known isotopes. P-31 is the only stable isotope.. It is colorless and transparent in its pure form. Phosphorus is insoluble in water, but soluble in carbon disulfide. Phosphorus burns spontaneously in air to its pentoxide. It is highly poisonous, with a lethal dose of ~50 mg. White phosphorus should be stored under water and handled with forceps. It causes severe burns when in contact with skin. White phosphorus is converted to red phosphorus when exposed to sunlight or heated in its own vapor to 250°C. Unlike white phosphorus, red phosphorus does not phosphoresce in air, although it still requires careful handling. Red phosphorus, which is relatively stable, is used to make safety matches, tracer bullets, incendiary devices, pesticides, pyrotechnic devices, and many other products. There is a high demand for phosphates for use as fertilizers. Phosphates are also used to make certain glasses (e.g., for sodium lamps). Trisodium phosphate is used as a cleaner , water softer, and scale/corrosion inhibitor. Bone ash (calcium phosphate) is used to make chinaware and to make monocalcium phosphate for baking powder. Phosphorus is used to make steels and phosphor bronze and is added to other alloys. There are many uses for organic phosphorus compounds. Phosphorus is an essential element in plant and animal cytoplasm. In humans, it is essential for proper skeletal and nervous system formation and function. Hennig Brand isolated phosphorus from urine. He kept his process a secret, choosing instead to sell the process to other alchemists. His process became more widely known when it was sold to the French Academy of Sciences. Phosphorus is the sixth most common element in the human body and it is also the seventh most common element in the Earth's crust.

Sixteen is Sulfur which is common nonmetal in volcanically active sites or volcanos Known since prehistoric time Brimstone is an ancient name for sulfur that means "burning stone". Sulfur is the seventeenth most common element in the Earth's crust., atomic symbol S atomic number 16 atomic weight 32.06 electron configuration [Ne] 3s2 3p4 Sulfur has a melting point of 112.8°C (rhombic) or 119.0°C (monoclinic), boiling point of 444.674°C, specific gravity of 2.07 (rhombic) or 1.957 (monoclinic) at 20°C, with a valence of 2, 4, or 6. Sulfur is a pale yellow, brittle, odorless solid. It is insoluble in water, but soluble in carbon disulfide. Multiple allotropes of sulfur are known. Sulfur has 21 known isotopes ranging from S-27 to S-46 and S-48. Four isotopes are stable: S-32, S-33, S-34 and S-36. S-32 is the most common isotope with an abundance of 95.02% Pure sulfur has no smell. The strong smell associated with sulfur should actually be attributed to compounds of sulfur. Sulfur is a component of gunpowder Gunpowder contains sulfur, carbon and saltpeter. It is used in the vulcanization of rubber. Sulfur has applications as a fungicide, fumigant, and in the making of fertilizers. It is used to make sulfuric acid. Sulfur is used in the making of several types of paper and as a bleaching agent. Elemental sulfur is used as an electrical insulator. The organic compounds of sulfur have many uses. Sulfur is an element that is essential for life. However, sulfur compounds can be highly toxic. For example, small amounts of hydrogen sulfide can be metabolized, but higher concentrations can quickly cause death from respiratory paralysis. Hydrogen sulfide quickly deadens the sense of smell. Sulfur dioxide is an important atmospheric pollutant. Sulfur is found in meteorites and native in proximity to hot springs and volcanoes. It is found in many minerals, including galena, iron pyrite, sphalerite, stibnite, cinnabar, Epsom salts, gypsum, celestite, and barite. Sulfur also occurs in petroleum crude oil and natural gas. The Frasch process may be used to obtain sulfur commercially. In this process, heated water is forced into wells sunk into salt domes in order to melt the sulfur. The water is then brought to the surface

Chlorine is the seventeenth element being a Halogen atomic number 17 atomic symbol Cl atomic weight 35.45 electron configuration [Ne] 3s2 3p5 16 known isotopes with atomic masses ranging from 31 to 46 amu. Cl-35 and Cl-37 are both stable isotopes with Cl-35 as the most abundant form (75.8%). Chlorine has a melting point of -100.98°C, boiling point of -34.6°C, density of 3.214 g/l, specific gravity of 1.56 (-33.6°C, with a valence of 1, 3, 5, or 7. Chlorine is a member of the halogen section of elements and directly combines with almost all of the other elements. Chlorine gas is classified as a greenish-yellow irritating gas, at high pressure or low temperature: red to clear. Chlorine is the 21st most abundant element in the Earth’s crust, chlorine figures prominently in many organic chemistry reactions, particularly in substitutions with hydrogen. The gas acts as an irritant for respiratory and other mucous membranes. The liquid form will burn the skin and humans can smell as low an amount as 3.5 ppm. A few breaths at a concentration of 1000 ppm is usually fatal or can be. Chlorine is used in many everyday products. It is used for disinfecting drinking water or used in the production of textiles, paper products, dyes, petroleum products, medicines, insecticides, disinfectants, foods, solvents, plastics, paints, and many other products. The element is used to manufacture chlorates, carbon tetrachloride, chloroform, and in the extraction of bromine. Chlorine has been it was used in chemical warfare. However naturein chlorine is only found in the combined state, most commonly with sodium as NaCl and in carnallite (KMgCl3•6H2O) and sylvite (KCl). The element is obtained from chlorides by electrolysis or via the action of oxidizing agents.

Argon being number eighteen as an Inert Gas atomic number 18 atomic symbol Ar atomic weight 39.94 electron configuration [Ne] 3s2 3p6 Argon has a freezing point of -189.2°C, boiling point of -185.7°C, and density of 1.7837 g/l. Argon is considered to be a noble or inert gas and does not form true chemical compounds, although it does form a hydrate with a dissociation pressure of 105 atm at 0°C. Ion molecules of argon have been observed, including (ArKr)+, (ArXe)+, and (NeAr)+. Argon forms a clathrate with b hydroquinone, which is stable yet without true chemical bonds.
Argon is two and a half times more soluble in water than nitrogen, with approximately the same solubility as oxygen. Argon's emission spectrumincludes a characteristic set of red lines. There are 22 known isotopes of argon ranging from Ar-31 to Ar-51 and Ar-53. Natural argon is a mixture of three stable isotopes: Ar-36 (0.34%), Ar-38 (0.06%), Ar-40 (99.6%). Ar-39 (half-life = 269 yrs) is to determine the age of ice cores, ground water and igneous rocks. Argon is used in electric lights and in fluorescent tubes, photo tubes, glow tubes, and in lasers. Argon is used as an inert gas for welding and cutting, blanketing reactive elements, and as a protective (nonreactive) atmosphere for growing crystals of silicon and germanium. Argon gas is prepared by Argon is produced commercially by fractional distillation of liquad air.. The Earth's atmosphere contains 0.94% argon. Mars' atmosphere contains 1.6% Argon-40 and 5 ppm Argon-36.

The nineteenth element is Potassium an alkali metal atomic symbol K atomic number 19 atomic weight 39.09 electron configuration [Ar]4s1 Potassium's melting point is 63.25°C, boiling point is 760°C, specific gravity is 0.862 (20°C), with a valence of 1. Three isotopes of potassium occur naturally on Earth, although at least 29 isotopes have been identified. The most abundant isotope is K-39, which accounts for 93.3% of the element. a radioactive isotope with a half-life of 1.28 x 109 years. Potassium is one of the most reactive and electropositive of metals. The only metal that is lighter than potassium is lithium. The soft, waxy, silvery-white metal (easily cut with a knife). The metal must be stored in a mineral oil, such as kerosene, as it oxidizes rapidly in air and catches fire spontaneously when exposed to water . Its decomposition in water evolves hydrogen. Potassium and its salts will color flames violet. Potash is in high demand as a fertilizer. Potassium, found in most soils, is an element that is essential for plant growth. An alloy of potassium and sodium is used as a heat transfer medium. Potassium salts have many commercial uses. Potassium is the 7th most abundant element on earth, making up 2.4% of the earth's crust, by weight. Potassium is not found free in nature. Potassium was the first metal isolated by electrolysis (Davy, 1807, from caustic potash KOH). Thermal methods (reduction of potassium compounds with C, Si, Na, CaC2) are also used to produce potassium. Sylvite, langbeinite, carnallite, and polyhalite form extensive deposits in ancient lake and sea beds, from which potassium salts can be obtained. In addition to other locations, potash is mined in Germany, Utah, California, and New Mexico. Because of its high reactivity, potassium is not found free in nature. It is formed by supernovas via the R-process and occurs on Earth dissolved in seawater and in ionic salts. Potassium was first purified in 1807 by Sir Humphry Davy from caustic potash (KOH) via electrolysis. Potassium was the first metal to be isolated using electrolysis. Potassium compounds emit a lilac or violet flame color when burned. It burns in water, just like sodium. The difference is that sodium burns with a yellow flame and is more likely to shatter and explode! When potassium burns in water, the reaction releases hydrogen gas. The heat of the reaction can ignite the hydrogen. The potassium ion is important for all living cells. Animals use sodium ions and potassium ions to generate electric potentials. This is vital for many cellular processes and is the basis for the conduction of nerve impulses and stabilization of blood pressure. When not enough potassium is available in the body, a potentially fatal condition called hypokalemia can occur. Symptoms of hypokalemia include muscle cramps and irregular heartbeat. An overabundance of potassium causes hypercalemia, which produces similar symptoms. Plants require potassium for many processes, so this element is a nutrient that is readily depleted by crops and must be replenished by fertilizers.

And the final element for this twenty element paper, Calcium which is the twentieth Alkaline Earth element on the periodic table atomic symbol Ca atomic number 20 atomic weight 40.07 electron configuration: [Ar]4s2

Calcium is essential for human nutrition. Animals skeletons get their rigidity primarily from calcium phosphate. The eggs of birds and shells of mollusks are comprised of calcium carbonate. Calcium is also necessary for plant growth. Calcium is used as a reducing agent when preparing metals from their halogen and oxygen compounds; as a reagent in purification of inert gases; to fix atmospheric nitrogen; as a scavenger and decarbonizer in metallurgy; and for making alloys. Calcium compounds are used in making lime, bricks, cement, glass, paint, paper, sugar, glazes, as well as for many other uses.