-
100
Carbon:C
pre-history It is used for the production of diamonds,it is versatile Carbon is the sixth most abundant element in the universe has been known since anciant times.Carbon is used mostly forcoal deposites. could not put N/A so i put the year 1000 -
100
Sulrfur:S
http://education.jlab.org/itselemental/ele016.html16SSulfur32.065
Atomic Number: 16
Atomic Weight: 32.065
Melting Point: 388.36 K (115.21°C or 239.38°F)
Boiling Point: 717.75 K (444.60°C or 832.28°F)
Density: 2.067 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Non-metal
Period Number: 3 Group Number: 16 Group Name: ChalcogenSulfur, the tenth most abundant element in the universe, has been known since ancient times. Sometime around 1777, Antoine Lavoisier convinced the rest of the scientific community -
500
Copper:Cu
http://education.jlab.org/itselemental/ele029.htmlIM PUTTING THEM IN Januery 1ST OK. 29CuCopper63.546
Atomic Number: 29
Atomic Weight: 63.546
Melting Point: 1357.77 K (1084.62°C or 1984.32°F)
Boiling Point: 2835 K (2562°C or 4644°F)
Density: 8.933 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 4 Group Number: 11 Group Name: none Archaeological evidence suggests that people have been using copper for at least 11,000 years. Relatively easy to mine and refine, people discovered method -
550
Gold:Au
Atomic Number: 79
Atomic Weight: 196.966569
Melting Point: 1337.33 K (1064.18°C or 1947.52°F)
Boiling Point: 3129 K (2856°C or 5173°F)
Density: 19.282 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 6 Group Number: 11 Group Name: none History and Uses: An attractive and highly valued metal, gold has been known for at least 5500 years. Gold is sometimes found free in nature but it is usually found in conjunction with silver, quartz -
550
Silver:Ag
47AgSilver107.8682
Atomic Number: 47
Atomic Weight: 107.8682
Melting Point: 1234.93 K (961.78°C or 1763.20°F)
Boiling Point: 2435 K (2162°C or 3924°F)
Density: 10.501 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 5 Group Number: 11 Group Name: none History and Uses: Archaeological evidence suggests that people have been using silver for at least 5000 years. Silver can be obtained from pure deposits, from silver ores such as argent -
Jan 1, 600
Iron:Fe
26FeIron55.845
Atomic Number: 26
Atomic Weight: 55.845
Melting Point: 1811 K (1538°C or 2800°F)
Boiling Point: 3134 K (2861°C or 5182°F)
Density: 7.874 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 4 Group Number: 8 Group Name: none History and Uses: Archaeological evidence suggests that people have been using iron for at least 5000 years. Iron is the cheapest and one of the most abundant of all metals, comprising nearly 5.6% of -
Jan 1, 650
Tin2:Sn
and is extracted by roasting cassiterite in a furnace with carbon. Tin makes up only about 0.001% of the earth's crust and is chiefly mined in Malaysia. Two allotropes of tin occur near room temperature. The first form of tin is called gray tin and is stable at temperatures below 13.2°C (55.76°F). There are few, if any, uses for gray tin. At temperatures above 13.2°C, gray tin slowly turns into tin's second form, white tin metal has many uses. -
Jan 1, 650
Tin3:Sn
Unfortunately, white tin will turn into gray tin if its temperature falls below 13.2°C. This change can be prevented if small amounts of antimony or bismuth are added to white tin. Tin resists corrosion and is used as a protective coating on other metals. Tin cans are probably the most familiar example of this application. A tin can is actually made from steel. A thin layer of tin is applied to the inside and outside of the can to keep the steel from rusting. -
Jan 1, 650
Tin4:Sn
Once widely used, tin cans have largely been replaced with plastic and aluminum containers. Tin is used in the Pilkington process to produce window glass. In the Pilkington process, molten glass is poured onto a pool of molten tin. The glass floats on the surface of the tin and cools, forming solid glass with flat, parallel surfaces. Most of the window glass produced today is made this way. Tin is used to form many useful alloys. Bronze is an alloy of tin and copper. -
Jan 1, 650
Tin1:Sn
50SnTin118.710
Atomic Number: 50
Atomic Weight: 118.710
Melting Point: 505.08 K (231.93°C or 449.47°F)
Boiling Point: 2875 K (2602°C or 4715°F)
Density: 7.287 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 5 Group Number: 14 Group Name: none History and Uses:
Archaeological evidence suggests that people have been using tin for at least 5500 years. Tin is primarily obtained from the mineral cassiterite (SnO2) -
Jan 1, 700
Antimony1:Sb
Atomic Number: 51
Atomic Weight: 121.760
Melting Point: 903.78 K (630.63°C or 1167.13°F)
Boiling Point: 1860 K (1587°C or 2889°F)
Density: 6.685 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Semi-metal
Period Number: 5 Group Number: 15 Group Name: Pnictogen History and Uses:
Antimony has been known since ancient times. It is sometimes found free in nature, but is usually obtained from the ores stibnite (Sb2S3) and valentinite (Sb2O3). Nicolas Lémery. -
Jan 1, 700
Antimony2:Sb
Nicolas Lémery, a French chemist, was the first person to scientifically study antimony and its compounds. He published his findings in 1707. Antimony makes up about 0.00002% of the earth's crust. Antimony is a brittle metal and is a poor conductor of heat and electricity. Very pure antimony is used to make certain types of semiconductor devices, such as diodes and infrared detectors. Antimony is alloyed with lead to increase lead's durability. Antimony alloys are also used in batteries, -
Jan 1, 750
Lead6:Pb
white lead. Lead chromate (PbCrO4), also known as crocoite, is used to produce chrome yellow paint. Lead nitrate (Pb(NO3)2) is used to make fireworks and other pyrotechnics. Lead silicate (PbSiO3) is used to make some types of glass and in the production of rubber and paints. -
Jan 1, 750
Lead1:Pb
82PbLead207.2
Atomic Number: 82
Atomic Weight: 207.2
Melting Point: 600.61 K (327.46°C or 621.43°F)
Boiling Point: 2022 K (1749°C or 3180°F)
Density: 11.342 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 6 Group Number: 14 Group Name: none History and Uses:
Lead has been known since ancient times. It is sometimes found free in nature, but is usually obtained from the ores galena (PbS), anglesite (PbSO4), cerussite (PbCO3) and minum -
Jan 1, 750
Lead3:Pb
lead is a cumulative poison and the decline of the Roman empire has been blamed, in part, on lead in the water supply. Lead is used to line tanks that store corrosive liquids, such as sulfuric acid (H2SO4). Lead's high density makes it useful as a shield against X-ray and gamma-ray radiation and is used in X-ray machines and nuclear reactors.Lead is also used as a covering on some wires and cables to protect them from corrosion, as a material to absorb vibrations and sounds. -
Jan 1, 750
Lead5:Pb
and plates. Babbit metal, another lead alloy, is used to reduce friction in bearings. Lead forms many useful compounds. Lead monoxide (PbO), also known as litharge, is a yellow solid that is used to make some types of glass, such as lead crystal and flint glass, in the vulcanizing of rubber and as a paint pigment. Lead dioxide (PbO2) is a brown material that is used in lead-acid storage batteries. Trilead tetraoxide (Pb3O4), also known as red lead, is used to make a reddish-brown paint. -
Jan 1, 750
Lead2:Pb
(Pb3O4). Although lead makes up only about 0.0013% of the earth's crust, it is not considered to be a rare element since it is easily mined and refined. Most lead is obtained by roasting galena in hot air, although nearly one third of the lead used in the United States is obtained through recycling efforts.Lead is a soft, malleable and corrosion resistant material. The ancient Romans used lead to make water pipes, some of which are still in use today. Unfortunately for the ancient Romans, -
Jan 1, 750
Lead4:Pb
and in the manufacture of ammunition. Most of the lead used today is used in the production on lead-acid storage batteries, such as the batteries found in automobiles. Several lead alloys are widely used. Solder, an alloy that is nearly half lead and half tin, is a material with a relatively low melting point that is used to join electrical components, pipes and other metallic items. Type metal, an alloy of lead, tin and antimony, is a material used to make the type used in printing presses. -
Jan 1, 1250
Arsenic2:As
in 1250. Arsenic occurs free in nature, but is most often found in the minerals arsenopyrite (FeAsS), realgar (AsS) and orpiment (As2S3). Today, most commercial arsenic is obtained by heating arsenopyrite.Arsenic and its compounds are poisonous. They have been used to make rat poison and some insecticides. Small amounts of arsenic are added to germanium to make transistors. Gallium arsenide (GaAs) can produce laser light directly from electricitricity. -
Jan 1, 1250
Arsenic1:As
Atomic Number: 33
Atomic Weight: 74.92160
Melting Point: 1090 K (817°C or 1503°F)
Boiling Point: 887 K (614°C or 1137°F)
Density: 5.776 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Semi-metal
Period Number: 4 Group Number: 15 Group Name: Pnictogen History and Uses: Although arsenic compounds were mined by the early Chinese, Greek and Egyptian civilizations, it is believed that arsenic itself was first identified by Albertus Magnus, a German alchemist -
Jan 1, 1500
Zinc3:Zn
protective coating of zinc. The zinc can be applied to an object by dipping it in a pool of molten zinc, but it is most often applied through an electroplating process. Sacrificial zinc anodes are used in cathodic protection systems to protect exposed iron from corrosion. Metallic zinc is also used to make dry cell batteries, roof cladding and die castings. -
Jan 1, 1500
Zinc4:Zn
Zinc is used to make many useful alloys. Brass, an alloy of zinc that contains between 55% and 95% copper, is probably the best known zinc alloy. Brass was first used about 2,500 years ago and was widely used by the ancient Romans, who used it to make such things as coins, kettles and decorative items. Brass is still used today, particularly in musical instruments, screws and other hardware that must resist corrosion. Zinc is alloyed with lead and tin to make solder, a metal with a relatively co -
Jan 1, 1500
Zinc:Zn
30ZnZinc65.38
Atomic Number: 30
Atomic Weight: 65.38
Melting Point: 692.68 K (419.53°C or 787.15°F)
Boiling Point: 1180 K (907°C or 1665°F)
Density: 7.134 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 4 Group Number: 12 Group Name: none History and Uses: Although zinc compounds have been used for at least 2,500 years in the production of brass, zinc wasn't recognized as a distinct element until much later. -
Jan 1, 1500
Zinc2:Zn
Metallic zinc was first produced in India sometime in the 1400s by heating the mineral calamine (ZnCO3) with wool. Zinc was rediscovered by Andreas Sigismund Marggraf in 1746 by heating calamine with charcoal. Today, most zinc is produced through the electrolysis of aqueous zinc sulfate (ZnSO4).Roughly one third of all metallic zinc produced today is used in a process known as galvanization. During galvanization, an object that is subject to corrosion, such as an iron nail, is given a continued -
Phosphorus2:P
filtering and otherwise processing as many as 60 buckets of urine. Thankfully, phosphorus is now primarily obtained from phosphate rock (Ca3(PO4)2).Phosphorus has three main allotropes: white, red and black. White phosphorus is poisonous and can spontaneously ignite when it comes in contact with air. For this reason, white phosphorus must be stored under water and is usually used to produce phosphorus compounds. -
Phosphorus3:P
Red phosphorus is formed by heating white phosphorus to 250°C (482°F) or by exposing white phosphorus to sunlight. Red phosphorus is not poisonous and is not as dangerous as white phosphorus, although frictional heating is enough to change it back to white phosphorus.Red phosphorus is used in safety matches, fireworks, smoke bombs and pesticides. Black phosphorus is also formed by heating white phosphorus, but a mercury catalyst and a seed crystal of black phosphorus are required. -
Phosphorus4:P
Black phosphorus is the least reactive form of phosphorus and has no significant commercial uses. Phosphoric acid (H3PO4) is used in soft drinks and to create many phosphate compounds, such as triple superphosphate fertilizer (Ca(H2PO4)2·H2O). Trisodium phosphate (Na3PO4) is used as a cleaning agent and as a water softener. Calcium phosphate (Ca3(PO4)2) is used to make china and in the production of baking powder. -
Phosphorus:P
Atomic Number: 15
Atomic Weight: 30.973762
Melting Point: 317.30 K (44.15°C or 111.47°F)
Boiling Point: 553.65 K (280.5°C or 536.9°F)
Density: 1.82 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Non-metal
Period Number: 3 Group Number: 15 Group Name: PnictogenHistory and Uses: In what is perhaps the most disgusting method of discovering an element, phosphorus was first isolated in 1669 by Hennig Brand, a German physician and alchemist, by boiling, -
Platinum:Pt
78PtPlatinum195.084
Atomic Number: 78
Atomic Weight: 195.084
Melting Point: 2041.55 K (1768.4°C or 3215.1°F)
Boiling Point: 4098 K (3825°C or 6917°F)
Density: 21.46 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 6 Group Number: 10 Group Name: none History and Uses: Used by the pre-Columbian Indians of South America, platinum wasn't noticed by western scientists until 1735. -
Platinum3:Pt
latinum is a soft, dense, ductile metal that is very resistant to corrosion. It is used to make jewelry, wire, electrical contacts and laboratory vessels. Platinum expands at nearly the same rate as soda-lime-silica glass, so it is used to make sealed electrodes in glass systems. Platinum is used to coat missile nose cones, jet engine fuel nozzles and other devices that must operate reliably for long periods of time at high temperatures. Platinum resistance wires are used in high temperature -
Platinum4:Pt
electric furnaces. Platinum anodes are used in cathodic protection systems to prevent ships, pipelines and steel piers from corroding in salt water. Platinum is widely used as a catalyst. It will convert methyl alcohol vapors (CH4O) into formaldehyde (CH2O) on contact, glowing red hot in the process.This effect is used to make small hand warmers. Platinum is also used in a device called a catalytic converter, a device found in the exhaust systems of most cars. -
Platinum2:Pt
Platinum can occur free in nature and is sometimes found in deposits of gold-bearing sands, primarily those found in the Ural mountains, Columbia and the western United States. Platinum, in the form of the mineral sperrylite (PtAs2), is also obtained as a byproduct of the nickel mining operation in the Sudbury region of Ontario, Canada. Credit for the modern rediscovery of platinum is usually given to Antonio de Ulloa. -
Nickel3:Ni
also used to manufacture some types of coins and batteries.Nickel is alloyed with other metals to improve their strength and resistance to corrosion. Nickel is alloyed with steel to make armor plate, vaults and machine parts. It is alloyed with copper to make pipes that are used in desalination plants. Very powerful permanent magnets, known as Alnico magnets, can be made from an alloy of aluminum, nickel, cobalt and iron. -
Nickel:Ni
Atomic Number: 28
Atomic Weight: 58.6934
Melting Point: 1728 K (1455°C or 2651°F)
Boiling Point: 3186 K (2913°C or 5275°F)
Density: 8.912 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 4 Group Number: 10 Group Name: noneHistory and Uses: Nickel was discovered by the Swedish chemist Axel Fredrik Cronstedt in the mineral niccolite (NiAs) in 1751. Today, most nickel is obtained from the mineral pentlandite (NiS·2FeS). Most of the cont -
Nickel2:Ni
world's supply of nickel is mined in the Sudbury region of Ontario, Canada. It is believed that this large deposit of nickel ore is a result of an ancient meteor impact.Nickel is a hard, corrosion resistant metal. It can be electroplated onto other metals to form a protective coating. Finely divided nickel is used as a catalyst for the hydrogenation of vegetable oils. Adding nickel to glass gives it a green color. A single kilogram of nickel can be drawn into 300 kilometers of wire. Nickel is -
Nitorgen2:N
of the earth's atmosphere, which contains an estimated 4,000 trillion tons of the gas. Nitrogen is obtained from liquefied air through a process known as fractional distillation.The largest use of nitrogen is for the production of ammonia (NH3). Large amounts of nitrogen are combined with hydrogen to produce ammonia in a method known as the Haber process. -
Nitrogen:N
7NNitrogen14.0067
Atomic Number: 7
Atomic Weight: 14.0067
Melting Point: 63.15 K (-210.00°C or -346.00°F)
Boiling Point: 77.36 K (-195.79°C or -320.44°F)
Density: 0.0012506 grams per cubic centimeter
Phase at Room Temperature: Gas
Element Classification: Non-metal
Period Number: 2 Group Number: 15 Group Name: PnictogenHistory and Uses: Nitrogen was discovered by the Scottish physician Daniel Rutherford in 1772. It is the fifth most abundant element in the universe and makes up about 78% -
Nitrogen3:N
Large amounts of ammonia are then used to create fertilizers, explosives and, through a process known as the Ostwald process, nitric acid (HNO3).Nitrogen gas is largely inert and is used as a protective shield in the semiconductor industry and during certain types of welding and soldering operations. Oil companies use high pressure nitrogen to help force crude oil to the surface. Liquid nitrogen is an inexpensive cryogenic liquid used for refrigeration, preservation of biological samples and for -
Oxygen3:O
Oxygen is the third most abundant element in the universe and makes up nearly 21% of the earth's atmosphere. Oxygen accounts for nearly half of the mass of the earth's crust, two thirds of the mass of the human body and nine tenths of the mass of water. Large amounts of oxygen can be extracted from liquefied air through a process known as fractional distillation. Oxygen can also be produced through the electrolysis of water or by heating potassium chlorate (KClO3). -
Chlorine:Cl
17ClChlorine35.453
Atomic Number: 17
Atomic Weight: 35.453
Melting Point: 171.65 K (-101.5°C or -150.7°F)
Boiling Point: 239.11 K (-34.04°C or -29.27°F)
Density: 0.003214 grams per cubic centimeter
Phase at Room Temperature: Gas
Element Classification: Non-metal
Period Number: 3 Group Number: 17 Group Name: HalogenHistory and Uses: Since it combines directly with nearly every element, chlorine is never found free in nature. -
Chlorine3:Cl
Chlorine is commonly used as an antiseptic and is used to make drinking water safe and to treat swimming pools. Large amounts of chlorine are used in many industrial processes, such as in the production of paper products, plastics, dyes, textiles, medicines, antiseptics, insecticides, solvents and paints. -
Oxygen2:O
Joseph Priestley and Carl Wilhelm Scheele both independently discovered oxygen, but Priestly is usually given credit for the discovery. They were both able to produce oxygen by heating mercuric oxide (HgO). Priestley called the gas produced in his experiments 'dephlogisticated air' and Scheele called his 'fire air'. The name oxygen was created by Antoine Lavoisier who incorrectly believed that oxygen was necessary to form all acids. -
Chlorine4:Cl
Two of the most familiar chlorine compounds are sodium chloride (NaCl) and hydrogen chloride (HCl). Sodium chloride, commonly known as table salt, is used to season food and in some industrial processes. Hydrogen chloride, when mixed with water (H2O), forms hydrochloric acid, a strong and commercially important acid. Other chlorine compounds include: chloroform (CHCl3), carbon tetrachloride (CCl4), potassium chloride (KCl), lithium chloride (LiCl), magnesium chloride (MgCl2) and chlorine dioxide -
Oxygen:O
Atomic Number: 8
Atomic Weight: 15.9994
Melting Point: 54.36 K (-218.79°C or -361.82°F)
Boiling Point: 90.20 K (-182.95°C or -297.31°F)
Density: 0.001429 grams per cubic centimeter
Phase at Room Temperature: Gas
Element Classification: Non-metal
Period Number: 2 Group Number: 16 Group Name: ChalcogenHistory and Uses: Oxygen had been produced by several chemists prior to its discovery in 1774, but they failed to recognize it as a distinct element. -
Chlorine2:Cl
Chlorine was first produced by Carl Wilhelm Scheele, a Swedish chemist, when he combined the mineral pyrolusite (MnO2) with hydrochloric acid (HCl) in 1774. Although Scheele thought the gas produced in his experiment contained oxygen, Sir Humphry Davy proved in 1810 that it was actually a distinct element. Today, most chlorine is produced through the electrolysis of aqueous sodium chloride (NaCl). -
Aluminum:Al
13AlAluminum26.9815386
Atomic Number: 13
Atomic Weight: 26.9815386
Melting Point: 933.437 K (660.323°C or 1220.581°F)
Boiling Point: 2792 K (2519°C or 4566°F)
Density: 2.70 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 3 Group Number: 13 Group Name: noneHistory and Uses: Although aluminum is the most abundant metal in the earth's crust, it is never found free in nature. All of the earth's aluminum has combined with other elements -
Aluminum2:Al
to form compounds. Two of the most common compounds are alum, such as potassium aluminum sulfate (KAl(SO4)2·12H2O), and aluminum oxide (Al2O3). About 8.2% of the earth's crust is composed of aluminum.Scientists suspected than an unknown metal existed in alum as early as 1787, but they did not have a way to extract it until 1825. Hans Christian Oersted, a Danish chemist, was the first to produce tiny amounts of aluminum. -
Aluminum3:Al
Two years later, Friedrich Wöhler, a German chemist, developed a different way to obtain aluminum. By 1845, he was able to produce samples large enough to determine some of aluminum's basic properties.Wöhler's method was improved in 1854 by Henri Étienne Sainte-Claire Deville, a French chemist. Deville's process allowed for the commercial production of aluminum. As a result, the price of aluminum dropped from around $1200 per kilogram in 1852 to around $40 per kilogram in 1859. Unfortunately, -
Aluminum4:Al
aluminum remained too expensive to be widely used.Two important developments in the 1880s greatly increased the availability of aluminum. The first was the invention of a new process for obtaining aluminum from aluminum oxide. Charles Martin Hall, an American chemist, and Paul L. T. Héroult, a French chemist, each invented this process independently in 1886. The second was the invention of a new process that could cheaply obtain aluminum oxide from bauxite.Bauxite is an ore that contains a large -
Fluorine:F
Atomic Number: 9
Atomic Weight: 18.9984032
Melting Point: 53.53 K (-219.62°C or -363.32°F)
Boiling Point: 85.03 K (-188.12°C or -306.62°F)
Density: 0.001696 grams per cubic centimeter
Phase at Room Temperature: Gas
Element Classification: Non-metal
Period Number: 2 Group Number: 17 Group Name: HalogenHistory and Uses: Fluorine is the most reactive of all elements and no chemical substance is capable of freeing fluorine from any of its compounds. For this reason, fluorine does not occur fr -
Fluorine3:F
in Gore's experiment when the fluorine gas that formed on one electrode combined with the hydrogen gas that formed on the other electrode. Ferdinand Frederic Henri Moissan, a French chemist, was the first to successfully isolate fluorine in 1886. He did this through the electrolysis of potassium fluoride (KF) and hydrofluoric acid (HF). He also completely isolated the fluorine gas from the hydrogen gas and he built his electrolysis device completely from platinum. His work was so impressive that -
Fluorine2:F
ee in nature and was extremely difficult for scientists to isolate. The first recorded use of a fluorine compound dates to around 1670 to a set of instructions for etching glass that called for Bohemian emerald (CaF2). Chemists attempted to identify the material that was capable of etching glass and George Gore was able to produce a small amount of fluorine through an electrolytic process in 1869.Unknown to Gore, fluorine gas explosively combines with hydrogen gas. That is exactly what happened -
Argon:Ar
Atomic Number: 18
Atomic Weight: 39.948
Melting Point: 83.80 K (-189.35°C or -308.83°F)
Boiling Point: 87.30 K (-185.85°C or -302.53°F)
Density: 0.0017837 grams per cubic centimeter
Phase at Room Temperature: Gas
Element Classification: Non-metal
Period Number: 3 Group Number: 18 Group Name: Noble GasHistory and Uses: Argon was discovered by Sir William Ramsay, a Scottish chemist, and Lord Rayleigh, an English chemist, in 1894. Argon makes up 0.93% of the earth's atmosphere, making it the -
Argon2:Ar
third most abundant gas. Argon is obtained from the air as a byproduct of the production of oxygen and nitrogen.Argon is frequently used when an inert atmosphere is needed. It is used to fill incandescent and fluorescent light bulbs to prevent oxygen from corroding the hot filament. Argon is also used to form inert atmospheres for arc welding, growing semiconductor crystals and processes that require shielding from other atmospheric gases.Once thought to be completely inert, argon is known to fo -
Argon3:Ar
rm at least one compound. The synthesis of argon fluorohydride (HArF) was reported by Leonid Khriachtchev, Mika Pettersson, Nino Runeberg, Jan Lundell and Markku Räsänen in August of 2000. Stable only at very low temperatures, argon fluorohydride begins to decompose once it warms above -246°C (-411°F). Because of this limitation, argon fluorohydride has no uses outside of basic scientific research. -
Heluim2:He
Pierre-Jules-César Janssen, a French astronomer, noticed a yellow line in the sun's spectrum while studying a total solar eclipse in 1868. Sir Norman Lockyer, an English astronomer, realized that this line, with a wavelength of 587.49 nanometers, could not be produced by any element known at the time.It was hypothesized that a new element on the sun was responsible for this mysterious yellow emission. This unknown element was named helium by Lockyer.The hunt to find helium on earth ended in 1895 -
Heluim3:He
on earth ended in 1895. Sir William Ramsay, a Scottish chemist, conducted an experiment with a mineral containing uranium called clevite. He exposed the clevite to mineral acids and collected the gases that were produced. He then sent a sample of these gases to two scientists, Lockyer and Sir William Crookes, who were able to identify the helium within it. Two Swedish chemists, Nils Langlet and Per Theodor Cleve, independently found helium in clevite at about the same time as Ramsay.Helium makes -
Heluim4:He
Helium makes up about 0.0005% of the earth's atmosphere.This trace amount of helium is not gravitationally bound to the earth and is constantly lost to space. The earth's atmospheric helium is replaced by the decay of radioactive elements in the earth's crust. Alpha decay, one type of radioactive decay, produces particles called alpha particles.An alpha particle can become a helium atom once it captures two electrons from its surroundings. This newly formed helium can eventually work its way to -
Heluim:He
Atomic Number: 2
Atomic Weight: 4.002602
Melting Point: 0.95 K (-272.2°C or -458.0°F)
Boiling Point: 4.22 K (-268.93°C or -452.07°F)
Density: 0.0001785 grams per cubic centimeter
Phase at Room Temperature: Gas
Element Classification: Non-metal
Period Number: 1 Group Number: 18 Group Name: Noble GasHistory and Uses: Helium, the second most abundant element in the universe, was discovered on the sun before it was found on the earth. -
Krpton:Kr
Atomic Number: 36
Atomic Weight: 83.798
Melting Point: 115.79 K (-157.36°C or -251.25°F)
Boiling Point: 119.93 K (-153.22°C or -243.80°F)
Density: 0.003733 grams per cubic centimeter
Phase at Room Temperature: Gas
Element Classification: Non-metal
Period Number: 4 Group Number: 18 Group Name: Noble GasHistory and Uses: Krypton was discovered on May 30, 1898 by Sir William Ramsay, a Scottish chemist, and Morris M. Travers, an English chemist, while studying liquefied air. Small amounts of -
Krpton2:Kr
liquid krypton remained behind after the more volatile components of liquid air had boiled away. The earth's atmosphere is about 0.0001% krypton.The high cost of obtaining krypton from the air has limited its practical applications. Krypton is used in some types of photographic flashes used in high speed photography. Some fluorescent light bulbs are filled with a mixture of krypton and argon gases. Krypton gas is also combined with other gases to make luminous signs that glow with a greenish-yel -
Neon:Ne
10NeNeon20.1797
Atomic Number: 10
Atomic Weight: 20.1797
Melting Point: 24.56 K (-248.59°C or -415.46°F)
Boiling Point: 27.07 K (-246.08°C or -410.94°F)
Density: 0.0008999 grams per cubic centimeter
Phase at Room Temperature: Gas
Element Classification: Non-metal
Period Number: 2 Group Number: 18 Group Name: Noble GasHistory and Uses: Neon was discovered by Sir William Ramsay, a Scottish chemist, and Morris M. Travers, an English chemist, shortly after their discovery of the element -
polonium2:Po
radioactive element. Curie needed to refine several tons of pitchblende in order to obtain tiny amounts of polonium and radium, another radioactive element discovered by Curie. One ton of uranium ore contains only about 100 micrograms (0.0001 grams) of polonium. Due to its scarcity, polonium is usually produced by bombarding bismuth-209 with neutrons in a nuclear reactor. This forms bismuth-210, which has a half-life of 5 days. Bismuth-210 decays into polonium-210 through beta decay. Milligram -
Radium:Ra
88RaRadium226
Atomic Number: 88
Atomic Weight: 226
Melting Point: 973 K (700°C or 1292°F)
Boiling Point: 1413 K (1140°C or 2084°F)
Density: 5 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 7 Group Number: 2 Group Name: Alkaline Earth Metal
RadioactiveHistory and Uses: Radium was discovered by Marie Sklodowska Curie, a Polish chemist, and Pierre Curie, a French chemist, in 1898. Marie Curie obtained radium from pitchblende, a materi -
Radium2:Ra
ial that contains uranium, after noticing that unrefinedpitchblende was more radioactive than the uranium that was separated from it. She reasoned that pitchblende must contain at least one other radioactive element. Curie needed to refine several tons of pitchblende in order to obtain tiny amounts of radium and polonium, another radioactive element discovered by CurieOne ton of uranium ore contains only about 0.14 grams of radium. Today, radium can be obtained as a byproduct of refining uranium -
Radium3:Ra
Radium's most stable isotope, radium-226, has a half-life of about 1600 years. It decays into radon-222 through alpha decay or into lead-212 by ejecting a carbon-14 nucleus. The Curie, a unit used to describe the activity of a radioactive substance, is based on radium-226. It is equal to the number of atoms in a one gram sample of radium-226 that will decay in one second, or 37,000,000,000 decays per second. -
polonium:Po
Atomic Number: 84
Atomic Weight: 209
Melting Point: 527 K (254°C or 489°F)
Boiling Point: 1235 K (962°C or 1764°F)
Density: 9.32 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 6 Group Number: 16 Group Name: Chalcogen
RadioactivePolonium was discovered by Marie Sklodowska Curie, a Polish chemist, in 1898. She obtained polonium from pitchblende, a material that contains uranium, after noticing that unrefined pitchblende was more radio -
Neon2:Ne
krypton in 1898. Like krypton, neon was discovered through the study of liquefied air. Although neon is the fourth most abundant element in the universe, only 0.0018% of the earth's atmosphere is neon.The largest use for neon gas is in advertising signs. Neon is also used to make high voltage indicators and is combined with helium to make helium-neon lasers. Liquid neon is used as a cryogenic refrigerant. Neon is highly inert and forms no known compounds, although there is some evidence that it -
Actinium:Ac
The Element Actinium
[Click for Isotope Data] 89AcActinium227
Atomic Number: 89
Atomic Weight: 227
Melting Point: 1324 K (1051°C or 1924°F)
Boiling Point: 3471 K (3198°C or 5788°F)
Density: 10.07 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 7 Group Number: none Group Name: Actinide
RadioactiveHistory and Uses: Actinium was discovered in 1899 by André-Louis Debierne, a French chemist, while experimenting with new methods of separ -
Actinium2:Ac
Actinium is a rare element that is present in uranium ores in tiny amounts, but it is usually cheaper and easier to create actinium when it is needed by bombarding radium with neutrons in a nuclear reactor. Actinium's most stable isotope, actinium-227, has a half-life of 21.77 years. It decays into francium-223 through alpha decay or into thorium-227 through beta decay. -
Radon:Rn
86RnRadon222
Atomic Number: 86
Atomic Weight: 222
Melting Point: 202 K (-71°C or -96°F)
Boiling Point: 211.45 K (-61.7°C or -79.1°F)
Density: 0.00973 grams per cubic centimeter
Phase at Room Temperature: Gas
Element Classification: Non-metal
Period Number: 6 Group Number: 18 Group Name: Noble Gas
RadioactiveHistory and Uses: Radon was discovered by Friedrich Ernst Dorn, a German chemist, in 1900 while studying radium's decay chain. Originally named niton after the Latin word for shining, -
Francium:Fr
87FrFrancium223
Atomic Number: 87
Atomic Weight: 223
Melting Point: 300 K (27°C or 81°F)
Boiling Point: Unknown
Density: Unknown
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 7 Group Number: 1 Group Name: Alkali Metal
RadioactiveFrancium was discovered by Marguerite Catherine Perey, a French chemist, in 1939 while analyzing actinium's decay sequence. Although considered a natural element, scientists estimate that there is no more than one ounce of francium i -
Francium2:Fr
Since there is so little naturally occurring francium on earth, scientists must produce francium in order to study it. Francium can be produced by bombarding thorium with protons or by bombarding radium with neutrons. -
plutonium:Pu
he Element Plutonium
[Click for Isotope Data] 94PuPlutonium244
Atomic Number: 94
Atomic Weight: 244
Melting Point: 913 K (640°C or 1184°F)
Boiling Point: 3501 K (3228°C or 5842°F)
Density: 19.84 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 7 Group Number: none Group Name: Actinide
Radioactive and Artificially ProducedPlutonium was first produced by Glenn T. Seaborg, Joseph W. Kennedy, Edward M. McMillan and Arthur C. Wohl by bomb -
Americium:Am
Atomic Number: 95
Atomic Weight: 243
Melting Point: 1449 K (1176°C or 2149°F)
Boiling Point: 2284 K (2011°C or 3652°F)
Density: 13.69 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 7 Group Number: none Group Name: Actinide
Radioactive and Artificially ProducedHistory and Uses: Americium was discovered in 1944 by the American scientists Glenn T. Seaborg, Ralph A. James, Leon O. Morgan and Albert Ghiorso. They produced americium by b -
Americium2:Am
bombarding plutonium-239, an isotope of plutonium, with high energy neutrons. This formed plutonium-240, which was itself bombarded with neutrons. The plutonium-240 changed into plutonium-241, which then decayed into americium-241 through beta decay. This work was carried out at the University of Chicago's Metallurgical Laboratory, now known as Argonne National Laboratory.Americium's most stable isotope, americium-243, has a half-life of about 7,370 years. It decays into neptunium-239 through a -
Dubnium:Db
Atomic Number: 105
Atomic Weight: 268
Melting Point: Unknown
Boiling Point: Unknown
Density: Unknown
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 7 Group Number: 5 Group Name: none
Radioactive and Artificially ProducedHistory and Uses: Scientists working at the Joint Institute for Nuclear Research in Dubna, Russia, first reported the production of dubnium in 1967. -
Vanadium:V
23VVanadium50.9415
Atomic Number: 23
Atomic Weight: 50.9415
Melting Point: 2183 K (1910°C or 3470°F)
Boiling Point: 3680 K (3407°C or 6165°F)
Density: 6.0 grams per cubic centimeter
Phase at Room Temperature: Solid
Element Classification: Metal
Period Number: 4 Group Number: 5 Group Name: noneHistory and Uses:
Vanadium was discovered by Andrés Manuel del Rio, a Mexican chemist, in 1801. Rio sent samples of vanadium ore and a letter describing his methods to the Institute de France in Paris -
Vanadium2:V
France, for analysis and confirmation. Unfortunately for Rio, his letter was lost in a shipwreck and the Institute only received his samples, which contained a brief note describing how much this new element, which Rio had named erythronium, resembled chromium. Rio withdrew his claim when he received a letter from Paris disputing his discovery. Vanadium was rediscovered by Nils Gabriel Sefstrôm, a Swedish chemist, in 1830 while analyzing samples of iron from a mine in Sweden. -
Vanadium3:V
Vanadium was rediscovered by Nils Gabriel Sefstrôm, a Swedish chemist, in 1830 while analyzing samples of iron from a mine in Sweden. Vanadium was isolated by Sir Henry Enfield Roscoe, an English chemist, in 1867 by combining vanadium trichloride (VCl3) with hydrogen gas (H2). Today, vanadium is primarily obtained from the minerals vanadinite (Pb5(VO)3Cl) and carnotite (K2(UO2)2VO4·1-3H2O) by heating crushed ore in the presence of carbon and chlorine to produce vanadium trichloride. -
Vanadium4:V
The vanadium trichloride is then heated with magnesium in an argon atmosphere. Vanadium is corrosion resistant and is sometimes used to make special tubes and pipes for the chemical industry. Vanadium also does not easily absorb neutrons and has some applications in the nuclear power industry. A thin layer of vanadium is used to bond titanium to steel.Nearly 80% of the vanadium produced is used to make ferrovanadium or as an additive to steel. Ferrovanadium is a strong, shock resistant. -
Period: to
The Elements
The Elements:gold,Dubnuim,Rodon,Americium,Francuim,Unubuim,silver,cooper,Neon,Argon,Heluim,Radium,Actinuim,Polonuim,Fluorine,Krpton,Carbon,Sulfur,Iron,Tin,Antimony,Lead,Arsenic,Zinc,Phosphere,Platinum,Nickle,Nitorgen,Oxygen,Chlorine,Aluminuim. YAY
