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Barium

Barium. Zong Peiyi G9R. Who discovered it???. Sir Humphry Davy An English chemist Discovered barium in the year 1808. It is not found freely but is only found in combination with other elements Also discovered potassium, sodium, boron and magnesium. How?.

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Barium

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  1. Barium Zong Peiyi G9R

  2. Who discovered it??? Sir Humphry Davy An English chemist Discovered barium in the year 1808. It is not found freely but is only found in combination with other elements Also discovered potassium, sodium, boron and magnesium

  3. How? Davy used a technique later to be called electrolysis The first time he produced pure barium, he did it by having an electric current pass through molten barium hydroxide.

  4. Introduction • Barium is the fourteenth most abundant element in the Earth’s crust. • Its abundance is estimated to be about 0.05 percent • The world’s major sources of barium ores are China, India, Morocco, the US, Turkey, and Kazakhstan • The most common sources of barium are barite and witherite. They are often found in nature as underground ore deposits

  5. Extraction • Pure barium is produced by reacting barium oxide with aluminum or silicon • Two forms of barium, barium sulfate and barium carbonate, are often found in nature as underground ore deposits • Barium is sometimes found naturally in drinking water and food.

  6. Reactions With air • Once ignited, barium metal burns in air to give a mixture of white barium oxide and barium nitride

  7. Reactions With water • Reacts readily to form barium hydroxide and hydrogen gas

  8. Reaction with Halogens Iodides BaI2.2H2O: barium (II) iodide BaI2: barium (II) iodide Oxides BaO: barium (II) oxide BaO2: barium (II) peroxide Sulfides BaS: barium (II) sulphide Selenides BaSe: barium (II) selenide Nitrides Ba3N2: barium nitride Hydrides BaH2: barium (II) hydride Fluorides BaF2: barium (II) fluoride Chlorides BaCl2: barium (II) chloride BaCl2.2H2O: barium (II) chloride Bromides BaBr2: barium (II) bromide BaBr2.2H2O: barium (II) bromide

  9. Properties • Pale yellow • Shiny • Malleable – capable of being hammered into thin sheets • Melting point - about 700°C • Boiling point – about 1500 °C • Density – 3.6 grams per cubic centimeter • When heated, barium compound give off a pale yellow-green flame. This property is used as a test for barium Physical

  10. Properties • Active metal • Combines easily with oxygen, the halogens, and other non-metals • Barium also reacts with water and with most acids • It is so reactive that it must be stored under kerosene, petroleum, or other oily liquid to prevent it from reacting with oxygen and moisture in the air Chemical

  11. Uses Few uses cause it is too reactive Used in fireworks to give a green coloration Used in glassmaking Used as a getter in the electronics industry, to remove the last traces of gases in vacuum tubes Used in medicine in the form of a Barium Meal Barium is used in X-rays by having a patient swallow a solution containing Barium. This solution will show up on the X-ray, and let the doctor trace your digestive track.

  12. How was it used initially? During the middle ages, witches and alchemists were attracted to them because after exposure to light they would glow for years They were known as “Bologna stones”

  13. Environmental Impacts Barium and all of its compounds are very toxic Some barium compounds that are released during industrial processes dissolve easily in water and are found in water bodies Because of their water-solubility these barium compounds can spread over great distances When fish and other aquatic organisms absorb the barium compounds, barium will accumulate in their bodies

  14. Health issues People that work in the barium industry will breathe in air that contains barium sulphate or barium carbonate Many hazardous waste sites contain certain amount of barium. People that live near them may be exposed to harmful levels Barium compounds that dissolve in water can be harmful to human health Small amounts of water-soluble barium may cause a person to experience breathing difficulties, increased blood pressures, heart rhythm changes, stomach irritation, muscle weakness, changes in nerve reflexes, swelling of brains and liver, kidney and heart damage The uptake of large amounts of barium that are water-soluble may cause paralyses and death

  15. FUTURE Health Issues Barium has not known to cause cancer to humans till then There are no proof that barium can cause infertility or birth defeats now

  16. Bibliography "Barium." Barium. N.p., n.d. Web. 12 Feb. 2014. <http://www.ucc.ie/academic/chem/dolchem/html/elem056.html>. "Barium." Wikipedia. Wikimedia Foundation, 13 Jan. 2014. Web. 12 Feb. 2014. <http://en.wikipedia.org/wiki/Barium#History>. "Barium - Ba." Barium (Ba). N.p., n.d. Web. 11 Feb. 2014. <http://www.lenntech.com/periodic/elements/ba.htm>. "What is barium used for today?." WikiAnswers. Answers Corporation, n.d. Web. 12 Feb. 2014. <http://wiki.answers.com/Q/What_is_barium_used_for_today>. Winter, Mark. "Barium  ." Chemistry : Periodic Table : barium : compounds information. N.p., 18 Apr. 2004. Web. 12 Feb. 2014. <http://jpkc.whut.edu.cn/web18/main/wangluo/webelements/webelements/elements/text/ba/comp.html>. "Chemistry Explained." Barium, Chemical Element. Admaveg, n.d. Web. 12 Feb. 2014. <http://www.chemistryexplained.com/elements/A-C/Barium.html>.

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